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All Textbook Solutions for Chemistry by OpenStax (2015-05-04)

Explain how you could experimentally determine whether the outside temperature is higher or lower than 0 oC (32 oF) without using a thermometer.Identify each of the following statements as being most similar to a hypothesis, a law, or a theory. Explain your reasoning. (a) Falling barometric pressure precedes the onset of bad weather. (b) All life on earth has evolved from a common, primitive organism through the process of natural selection. (c) My truck’s gas mileage has dropped significantly, probably because it’s due for a tune-up.Identify each of the following statements as being most similar to a hypothesis, a law, or a theory. Explain your reasoning. (a) The pressure of a sample of gas is directly proportional to the temperature of the gas. (b) Matter consists of tiny particles that can combine in specific ratios to form substances with specific properties. (c) At a higher temperature, solids (such as salt or sugar) will dissolve better in water.Identify each of the underlined items as a part of either the macroscopic domain, the microscopic domain, or the symbolic domain of chemistry. For any in the symbolic domain, indicate whether they are symbols for a macroscopic or a microscopic feature. (a) The mass of a lead pipe is 14 lb. (b) The mass of a certain chlorine atom is 35 amu. (c) A bottle with a label that reads A] contains aluminum metal.Identify each of the underlined items as a part of either the macroscopic domain, the microscopic domain, or the symbolic domain of chemistry. For those in the symbolic domain, indicate whether they are symbols for a macroscopic or a microscopic feature. (a) A certain molecule contains one H atom and one Cl atom. (b) Copper wire has a density of about 8g/cm3. (c) The bottle contains 15 grams of Ni powder. (d) A sulfur molecule is composed of eight sulfur atoms.According to one theory, the pressure of a gas increases as its volume decreases because the molecules in the gas have to move a shorter distance to hit the walls of the container. Does this theory follow a macroscopic or microscopic description of chemical behavior? Explain your answer.The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.Why do we use an objects mass, rather than its weight, to indicate the amount of matter it contains?What properties distinguish solids from liquids? Liquids from gases? Solids from gases?How does a heterogeneous mixture differ from a homogeneous mixture? How are they similar?How does a homogeneous mixture differ from a pure substance? How are they similar?How does an element differ from a compound? How are they similar?How do molecules of elements and molecules of compounds differ? In what ways are they similar?How does an atom differ from a molecule? In what ways are they similar?Many of the items you purchase are mixtures of pure compounds. Select three of these commercial products and prepare a list of the ingredients that are pure compounds.Classify each of the following as an element, a compound, or a mixture: (a) copper (b) water (c) nitrogen (d) sulfur (e) air (f) sucrose (g) a substance composed of molecules each of which contains two iodine atoms (h) gasoline Classify each of the following as an element, a compound, or a mixture: iron oxygen mercury oxide pancake syrup carbon dioxide a substance composed of molecules each of which contains one hydrogen atom and one chlorine atom baking soda baking powder A sulfur atom and a sulfur molecule are not identical. What is the difference?How are the molecules in oxygen gas, the molecules in hydrogen gas, and water molecules similar? How do they differ?We refer to astronauts in space as weightless, but not without mass. Why?As we drive an automobile, we don’t think about the chemicals consumed and produced. Prepare a list of the principal chemicals consumed and produced during the operation of an automobile.Matter is everywhere around us. Make a list by name of fifteen different kinds of matter that you encounter every day. Your list should include (and label at least one example of each) the following: a solid, a liquid, a gas, an element, a compound, a homogenous mixture, a heterogeneous mixture, and a pure substance.When elemental iron corrodes it combines with oxygen in the air to ultimately form red brown iron(III) oxide which we call rust. (a) If a shiny iron nail with an initial mass of 23.2 g is weighed after being coated in a layer of rust, would you expect the mass to have increased, decreased, or remained the same? Explain. (b) If the mass of the iron nail increases to 24.1 g, what mass of oxygen combined with the iron?As stated in the text, convincing examples that demonstrate the law of conservation of matter outside of the laboratory are few and far between. Indicate whether the mass would increase, decrease, or stay the same for the following scenarios where chemical reactions take place: Exactly one pound of bread dough is placed in a baking tin. The dough is cooked in an oven at 350 F releasing a wonderful aroma of freshly baked bread during the cooking process. Is the mass of the baked loaf less than, greater than, or the same as the one pound of original dough? Explain. When magnesium burns in air a white flaky ash of magnesium oxide is produced. Is the mass of magnesium oxide less than, greater than, or the same as the original piece of magnesium? Explain. Antoine Lavoisier, the French scientist credited with first stating the law of conservation of matter, heated a mixture of tin and air in a sealed flask to produce tin oxide. Did the mass of the sealed flask and contents decrease, increase, or remain the same after the heating Yeast converts glucose to ethanol and carbon dioxide during anaerobic fermentation as depicted in the simple chemical equation here: glucose ethanol + carbon dioxide If 200.0 g of glucose is fully converted, what will be the total mass of ethanol and carbon dioxide produced If the fermentation is carried out in an open container, would you expect the mass of the container and contents after fermentation to be less than, greater than, or the same as the mass of the container and contents before fermentation? Explain. If 97.7 g of carbon dioxide is produced, what mass of ethanol is produced Classify the six underlined properties in the following paragraph as chemical or physical: Fluorine is a pale yellow gas that reacts with most substances. The free element melts at 220 C and boils at 188 C. Finely divided metals burn in fluorine with a bright flame. Nineteen grams of fluorine will react with 1.0 gram of hydrogen.Classify each of the following changes as physical or chemical: condensation of steam burning of gasoline souring of milk dissolving of sugar in water melting of gold Classify each of the following changes as physical or chemical: coal burning ice melting mixing chocolate syrup with milk explosion of a firecracker magnetizing of a screwdriver The volume of a sample of oxygen gas changed from 10 mL to 11 mL as the temperature changed. Is this a chemical or physical change?A 2.0-mer volume of hydrogen gas combined with 1.0 liter of oxygen gas to produce 2.0 liters of water vapor. Does oxygen undergo a chemical or physical change?Explain the difference between extensive properties and intensive properties.Identify the following properties as either extensive or intensive. volume temperature humidity heat boiling point The density (d) of a substance is an intensive property that is defined as the ratio of its mass (m) to its volume (V).density=massvolumed=mV Considering that mass and volume are both extensive properties, explain why their ratio, density, is intensive.Is one liter about an ounce, a pint, a quart, or a gallon?Is a meter about an inch, a foot, a yard, or a mile?Indicate the SI base units or derived units that are appropriate for the following measurements: the length of a marathon race (26 miles 385 yards) the mass of an automobile the volume of a swimming pool the speed of an airplane the density of gold the area of a football field the maximum temperature at the South Pole on April 1, 1913 Indicate the SI base units or derived units that are appropriate for the following measurements: the mass of the moon the distance from Dallas to Oklahoma City the speed of sound the density of air the temperature at which alcohol boils the area of the state of Delaware the volume of a flu shot or a measles vaccination Give the name and symbol of the prefixes used with SI units to indicate multiplication by the following exact quantities. 103 102 0.1 103 1,000,000 0.000001 Give the name of the prefix and the quantity indicated by the following symbols that are used with ST base units. c d G k m n p T A large piece of jewelry has a mass of 132.6 g. A graduated cylinder initially contains 48.6 mL water. When the jewelry is submerged in the graduated cylinder, the total volume increases to 61.2 mL. Determine the density of this piece of jewelry. Assuming that the jewelry is made from only one substance, what substance is it likely to be? Explain.Visit this PhET density simulation (http://openstaxcollege.org/l/16phetmasvolden) and select the Same Volume Blocks. What are the mass, volume, and density of the yellow block What are the mass, volume and density of the red block List the block colors in order from smallest to largest mass. List the block colors in order from lowest to highest density. How are mass and density related for blocks of the same volume Visit this PhET density simulation (http://openstaxcollege.org/l/16phetmasvolden) and select Custom Blocks and then My Block. Enter mass and volume values for the block such that the mass in kg is less than the volume in L. What does the block do? Why? Is this always the case when mass < volume Enter mass and volume values for the block such that the mass in kg is more than the volume in L. What does the block do? Why? Is this always the case when mass > volume How would (a) and (b) be different if the liquid in the tank were ethanol instead of water How would (a) and (b) be different if the liquid in the tank were mercury instead of water Visit this PhET density simulation (http://openstaxcollege.org/l/16phetmasvolden) and select Mystery Blocks. Pick one of the Mystery Blocks and determine its mass, volume, density, and its likely identity. Pick a different Mystery Block and determine its mass, volume, density, and its likely identity. Order the Mystery Blocks from least dense to most dense. Explain.Express each of the following numbers in scientific notation with correct significant figures: 711.0 0.239 90743 134.2 0.05499 10000.0 0.000000738592 Express each of the following numbers in exponential notation with correct significant figures: 704 0.03344 547.9 22086 1000.00 0.0000000651 0.007157 Indicate whether each of the following can be determined exactly or must be measured with some degree of uncertainty: the number of eggs in a basket the mass of a dozen eggs the number of gallons of gasoline necessary to fill an automobile gas tank the number of cm in 2 m the mass of a textbook the time required to drive from San Francisco to Kansas City at an average speed of 53 mi/h Indicate whether each of the following can be determined exactly or must be measured with some degree of uncertainty: the number of seconds in an hour the number of pages in this book the number of grams in your weight the number of grams in 3 kilograms the volume of water you drink in one day the distance from San Francisco to Kansas City How many significant figures are contained in each of the following measurements? 38.7 g 21018m 3,486,002 kg 9.74150104J 0.0613cm3 17.0 kg 0.01400 g/mL How many significant figures are contained in each of the following measurements? 53 cm 2.05108m 86,002 J 9.740104m/s 10.0613m3 0.17 g/mL 0.88400 s The following quantities were reported on the labels of commercial products. Determine the number of significant figures in each. 0.0055 g active ingredients 12 tablets 3% hydrogen peroxide 5.5 ounces 473 mL 1.75% bismuth 0.00 1% phosphoric acid 99.80% inert ingredients Round off each of the following numbers to two significant figures: 0.436 9.000 27.2 135 1.497103 0.445 Round off each of the following numbers to two significant figures: 517 86.3 6.382103 5.0008 22.497 0.885 Perform the following calculations and report each answer with the correct number of significant figures. 628342 (5.63102)(7.4103) 28.013.483 81190.000023 14.98+27,340+84.7593 42.7+0.259 Perform the following calculations and report each answer with the correct number of significant figures. 62.834 0.147+0.0066+0.012 38951.792 150.150.6155 8.78(0.05000.478) 140+7.68+0.014 28.70.0483 (88.587.57)45.13 Consider the results of the archery contest shown in this figure. Which archer is most precise Which archer is most accurate Who is both least precise and least accurate Classify the following sets of measurements as accurate, precise, both, or neither. Checking for consistency in the weight of chocolate chip cookies: 17.27 g, 13.05 g, 19.46 g, 16.92 g Testing the volume of a batch of 25-mL pipettes: 27.02 mL, 26.99 mL, 26.97 mL, 27.01 mL Determining the purity of gold: 99.9999%, 99.9998%, 99.9998%, 99.9999%Write conversion factors (as ratios) for the number of: yards in 1 meter liters in 1 liquid quart pounds in 1 kilogram Write conversion factors (as ratios) for the number of: kilometers in 1 mile liters in 1 cubic foot grams in 1 ounce The label on a soft drink boule gives the volume in two units: 2.0 L and 67.6 fl oz. Use this information to derive a conversion factor between the English and metric units. How many significant figures can you justify in your conversion factor?The label on a box of cereal gives the mass of cereal in two units: 978 grams and 34.5 oz. Use this information to find a conversion factor between the English and metric units. How many significant figures can you justify in your conversion factor?Soccer is played with a round ball having a circumference between 27 and 28 in. and a weight between 14 and 16 oz. What are these specifications in units of centimeters and grams?A woman’s basketball has a circumference between 28.5 and 29.0 inches and a maximum weight of 20 ounces (two significant figures), What are these specifications in units of centimeters and grams?How many milliliters of a soft drink are contained in a 12.0-oz can?A barrel of oil is exactly 42 gal. How many liters of oil are in a barrel?The diameter of a red blood cell is about 3104 in. What is its diameter in centimeters?The distance between the centers of the two oxygen atoms in an oxygen molecule is 1.21108 cm. What is this distance in inches?Is a 197-lb weight lifter light enough to compete in a class limited to those weighing 90 kg or less?A very good 197-Ib weight lifter lifted 192 kg in a move called the clean and jerk. What was the mass of the weight lifted in pounds?Many medical laboratory tests are run using 5.0 L blood serum. What is this volume in milliliters?If an aspirin tablet Contains 325 mg aspirin, how many grams of aspirin does it contain?Use scientific (exponential) notation to express the following quantities in terms of the SI base units In Table 1.3: 0. 13 g 232 Gg 5.23 pm 86.3 mg 37.6 cm 54 m 1 Ts 27 ps 0.15 mK Complete the following conversions between SI units. 612g = mg 8.160 m ______ cm 3779 g = ________ g 781 mL = ______ L 4.18 kg = g 27.8 m = ______ km 0.13 mL = ______ L 1738 km ______ m 1.9 Gg = g Gasoline is sold by the liter in many countries. How many liters are required to fill a 12.0-gal gas tank?Milk is sold by the liter in many Countries. What is the volume of exactly 1/2 gal of milk in liters?A long ton is defined as exactly 2240 lb. What is this mass in kilograms?Make the conversion indicated in each of the following: the men’s world record long jump, 29 ft 414 in., to meters the greatest depth of the ocean, about 6.5 mi, to kilometers the area of the state of Oregon, 96,981 mi2 , to square kilometers the volume of 1 gill (exactly 4 oz) to milliliters the estimated volume of the oceans, 330,000,000 mi3 , to cubic kilometers. the mass of a 3525-lb car to kilograms the mass of a 2.3-oz egg to grams Make the conversion indicated in each of the following: the length of a soccer field, 120 m (three significant figures), to feet the height of Mt. Kilimanjaro, at 19,565 ft the highest mountain in Africa, to kilometers the area of an 8.5 × 11-inch sheet of paper in cm2 the displacement volume of an automobile engine, 161 in.3, to liters the estimated mass of the atmosphere, 5.61015 tons, to kilograms the mass of a bushel of rye, 32.0 lb, to kilograms the mass of a 5.00-grain aspirin tablet to milligrams (1 grain = 0.00229 oz)Many chemistry conferences have held a 50-Trillion Angstrom Run (two significant figures). How long is this run in kilometers and in miles? (1=11010m)Many chemistry conferences have held a 50-Trillion Angstrom Run (two significant figures). How long is this run in kilometers and in miles? (1=11010m) 79. A chemist’s 50-Trillion Angstrom Run (see Exercise 1.78) would be an archeologist’s 10,900 cubit run. How long is one cubit in meters and in feet? (1=1108cm)The gas tank of a certain luxury automobile holds 22.3 gallons according to the owner’s manual. If the density of gasoline is 0.8206 g/mL, determine the mass in kilograms and pounds of the fuel in a full tank.As an instructor is preparing for an experiment, he requires 225 g phosphoric acid. The only container readily available is a 150-mL Erlenmeyer flask. Is it large enough to contain the acid, whose density is 1.83 g/mL?To prepare for a laboratory period, a student lab assistant needs 125 g of a compound. A bottle containing 1/4 lb is available. Did the student have enough of the compound?A chemistry student is 159 cm tall and weighs 45.8 kg. What is her height in inches and weight in pounds?In a recent Grand Prix, the winner completed the race with an average speed of 229.8 km/h. What was his speed in miles per hour, meters per second, and feet per second?Solve these problems about lumber dimensions. To describe to a European how houses are constructed in the US, the dimensions of two-by-four lumber must be converted into metric units. The thickness × width × length dimensions are 1.50 in. × 3.50 in. × 8.00 ft in the US. What are the dimensions in cm × cm × m This lumber can be used as vertical studs, which are typically placed 16.0 in. apart. What is that distance in centimeters The mercury content of a stream was believed to be above the minimum considered safe —1 part per billion (ppb) by weight. An analysis indicated that the concentration was 0.68 parts per billion. What quantity of mercury in grams was present in 15.0 L of the water, the density of which is 0.998 g/ml? ( 1ppbHg=1ngHg1gwater)Calculate the density of aluminum if 27.6 cm3 has a mass of 74.6 g.Osmium is one of the densest elements known. What is its density if 2.72 g has a volume of 0.12 1 cm3?Calculate these masses. What is the mass of 6.00 cm3 of mercury, density = 13.5939 g/cm3 What is the mass of 25.0 mL octane, density = 0.702 g/cm3 Calculate these masses. What is the mass of 4.00 cm3 of sodium, density = 0.97 g/cm3 What is the mass of 125 mL gaseous chlorine, density = 3.16 g/L Calculate these volumes. What is the volume of 25 g iodine, density = 4.93 g/cm3 What is the volume of 3.28 g gaseous hydrogen, density = 0.089 g/L Calculate these volumes. What is the volume of 11.3 g graphite, density = 2.25 g/cm3 What is the volume of 39.657 g bromine, density = 2.928 g/cm3 Convert the boiling temperature of gold, 2966 C, into degrees Fahrenheit and kelvin.Convert the temperature of scalding water, 54 C, into degrees Fahrenheit and kelvin.Convert the temperature of the coldest area in a freezer, 10 F, to degrees Celsius and kelvin.Convert the temperature of dry ice, 77 C, into degrees Fahrenheit and kelvin.Convert the boiling temperature of liquid ammonia. 28.1 F, into degrees Celsius and kelvin.The label on a pressurized can of spray disinfectant warns against heating the can above 130 F. What are the corresponding temperatures on the Celsius and kelvin temperature scales?The weather in Europe was unusually warm during the summer of 1995. The TV news reported temperatures as high as 45 C. What was the temperature on the Fahrenheit scale?In the following drawing, the green spheres represent atoms of a certain element. The purple spheres represent atoms of another element. If the spheres of different elements touch, they are part of a single unit of a compound. The following chemical change represented by these spheres may violate one of the ideas of Dalton’s atomic theory. Which one?Which postulate of Dalton’s theory is consistent with the following observation concerning the weights of reactants and products? When loo grams of solid calcium carbonate is heated, 44 grams of carbon dioxide and 56 grams of calcium oxide are produced.Identify the postulate of Dalton’s theory that is violated by the following observations: 59.95% of one sample of titanium dioxide is titanium; 60.10% of a different sample of titanium dioxide is titanium.Samples of compound X, Y, and Z are analyzed, with results shown here. Compound Description Mass of Carbon Mass of Hydrogen X clear, colorless, liquid with strong odor 1.776 g 0.148 g Y clear, colorless, liquid with strong odor 1.974 g 0.329 g Z clear, colorless, liquid with strong odor 7.812 g 0.651 g Do these data provide example(s) of the law of definite proportions, the law of multiple proportions, neither, or both? What do these data tell you about compounds X, Y, and Z?The existence of isotopes violates one of the original ideas of Dalton’s atomic theory. Which one?How are electrons and protons similar? How are they different?How are protons and neutrons similar? How are they different?Predict and test the behavior of a particles fired at a plum pudding model atom. Predict the paths taken by a particles that are fired at atoms with a Thomson’s plum pudding model structure. Explain why you expect the particles to take these paths. If a particles of higher energy than those in (a) are fired at plum pudding atoms, predict how their paths will differ from the lower-energy a particle paths. Explain your reasoning. Now test your predictions from (a) and (b). Open the Rutherford Scattering simulation (http://openstaxcollege.org/I/16PhetScatter) and select the Plum Pudding Atom tab. Set Alpha Particles Energy to mm, and select show traces. Click on the gun to start firing a particles. Does this match your prediction from (a)? If not, explain why the actual path would be that shown in the simulation. Hit the pause button, or Reset All. Set Alpha Particles Energy to max, and start firing a particles. Does this match your prediction from (b)? If not, explain the effect of increased energy on the actual paths as shown in the simulation.Predict and test the behavior of a particles fired at a Rutherford atom model. Predict the paths taken by a particles that are fired at atoms with a Rutherford atom model structure. Explain why you expect the particles to take these paths. If a particles of higher energy than those in (a) are fired at Rutherford atoms, predict how their paths will differ from the lower-energy a particle paths. Explain your reasoning. Predict how the paths taken by the particles will differ if they are fired at Rutherford atoms of elements other than gold. What factor do you expect to cause this difference in paths, and why? Now test your predictions from (a), (b), and (c). Open the Rutherford Scattering simulation (http://openstaxcollege.org/I/16PhetScatter) and select the Rutherford Atom tab. Due to the scale of the simulation, it is best to start with a small nucleus, so select 20 for both protons and neutrons, mm for energy, show traces, and then start firing a particles. Does this match your prediction from (a)? If not, explain why the actual path would be that shown in the simulation. Pause or reset, set energy to max, and start firing a particles. Does this match your prediction from (b)? If not, explain the effect of increased energy on the actual path as shown in the simulation. Pause or reset, select 40 for both protons and neutrons, mm for energy, show traces, and fire away. Does this match your prediction from (c)? If not, explain why the actual path would be that shown in the simulation. Repeat this with larger numbers of protons and neutrons. What generalization can you make regarding the type of atom and effect on the path of a particles? Be clear and specific.In what way are isotopes of a given element always different? In what way(s) are they always the same?Write the symbol for each of the following ions: the ion with a 1+ charge, atomic number 55, and mass number 133 the ion with 54 electrons, 53 protons, and 74 neutrons the ion with atomic number 15, mass number 31, and a 3 charge the ion with 24 electrons, 30 neutrons, and a 3+ charge Write the symbol for each of the following ions: the ion with a 3+ charge, 28 electrons, and a mass number of 71 the ion with 36 electrons, 35 protons, and 45 neutrons the ion with 86 electrons, 142 neutrons, and a 4+ charge the ion with a 2+ charge, atomic number 38, and mass number 87 Open the Build an Atom simulation (http://openstaxcollege.org/I/16PhetAtomBld) and click on the Atom icon. Pick any one of the first 10 elements that you would like to build and state its symbol. Drag protons, neutrons, and electrons onto the atom template to make an atom of your element. State the numbers of protons, neutrons, and electrons in your atom, as well as the net charge and mass number. Click on Net Charge and Mass Number, check your answers to (b), and correct, if needed. Predict whether your atom will be stable or unstable. State your reasoning. Check the Stable/Unstable box. Was your answer to (d) correct? If not, first predict what you can do to make a stable atom of your element, and then do it and see if it works. Explain your reasoning.Open the Build an Atom simulation (http://openstaxcollege.org/l/16PhetAtomBld) Drag protons, neutrons, and electrons onto the atom template to make a neutral atom of Oxygen-16 and give the isotope symbol for this atom. Now add two more electrons to make an ion and give the symbol for the ion you have created.Open the Build an Atom simulation (http://openstaxcollege.org/l/16PhetAtomBld) Drag protons, neutrons, and electrons onto the atom template to make a neutral atom of Lithium-6 and give the isotope symbol for this atom. Now remove one electron to make an ion and give the symbol for the ion you have created.Determine the number of protons, neutrons, and electrons in the following isotopes that are used in medical diagnoses: atomic number 9, mass number 18, charge of 1 atomic number 43, mass number 99, charge of 7+ atomic number 53, atomic mass number 131, charge of 1 atomic number 81, atomic mass number 201, charge of 1+ Name the elements in parts (a), (b), (c), and (d).The following are properties of isotopes of two elements that are essential in our diet. Determine the number of protons, neutrons and electrons in each and name them. atomic number 26, mass number 58, charge of 2+ atomic number 53, mass number 127, charge of 1 Give the number of protons, electrons, and neutrons in neutral atoms of each of the following isotopes: 510B 80199Hg 2963Ag 613N 3477P Give the number of protons, electrons, and neutrons in neutral atoms of each of the following isotopes: 37Li 52125Te 47109Ag 715N 1531P Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the Mix Isotopes tab, hide the Percent Composition and Average Atomic Mass boxes, and then select the element boron. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible.Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the Mix Isotopes tab, hide the Percent Composition and Average Atomic Mass boxes, and then select the element boron. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible. 21. Repeat Exercise 2.20 using an element that has three naturally occurring isotopes.An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element.Average atomic masses listed by JUPAC are based on a study of experimental results. Bromine has two isotopes 79Br and 81Br, whose masses (78.9 183 and 80.9 163 amu) and abundances (50.69% and 49.3 1%) were determined in earlier experiments. Calculate the average atomic mass of bromine based on these experiments.Variations in average atomic mass may be observed for elements obtained from different sources. Lithium provides an example of this. The isotopic composition of lithium from naturally occurring minerals is 7.5% 6Li and 92.5% 7Li, which have masses of 6.01512 amu and 7.01600 amu, respectively. A commercial source of lithium, recycled from a military source, was 3.75% 6Li (and the rest 7Li). Calculate the average atomic mass values for each of these two sources.The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.The 18O:16O abundance ratio in some meteorites is greater than that used to calculate the average atomic mass of oxygen on earth. Is the average mass of an oxygen atom in these meteorites greater than, less than, or equal to that of a terrestrial oxygen atom?Explain why the symbol for an atom of the element oxygen and the formula for a molecule of oxygen differ.Explain why the symbol for the element sulfur and the formula for a molecule of sulfur differ.Write the molecular and empirical formulas of the following compounds:Write the molecular and empirical formulas of the following compounds:Determine the empirical formulas for the following compounds: (a) caffeine, C8H10N4O2 (b) fructose, C12H22O11 (c) hydrogen peroxide, H2O2 (d) glucose, C6H12O6 (e) ascorbic acid (vitamin C), C6H8O6 Determine the empirical formulas for the following compounds: (a) acetic acid, C2H4O2 (b) citric acid, C6H8O7 (c) hydrazine, N2H4 (d) nicotine, C10H14N2 (e) butane, C4H10 Write the empirical formulas for the following compounds:Open the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) and select the Larger Molecules tab. Select an appropriate atoms Kit to build a molecule with two carbon and six hydrogen atoms. Drag atoms into the space above the Kit to make a molecule. A name will appear when you have made an actual molecule that exists (even if it is not the one you want). You can use the scissors tool to separate atoms if you would like to change the connections. Click on 3D to see the molecule, and look at both the space-filling and ball-and-stick possibilities. Draw the structural formula of this molecule and state its name. Can you arrange these atoms in any way to make a different compound?Open the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) and select the Larger Molecules tab. Select an appropriate atoms Kit to build a molecule with two carbon and six hydrogen atoms. Drag atoms into the space above the Kit to make a molecule. A name will appear when you have made an actual molecule that exists (even if it is not the one you want). You can use the scissors tool to separate atoms if you would like to change the connections. Click on 3D to see the molecule, and look at both the space-filling and ball-and-stick possibilities. Draw the structural formula of this molecule and state its name. Can you arrange these atoms in any way to make a different compound? 35. Use the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) to repeat Exercise 2.34, but build a molecule with two carbons, six hydrogens, and one oxygen. Draw the structural formula of this molecule and state its name. Can you arrange these atoms to make a different molecule? If so, draw its structural formula and state its name. How are the molecules drawn in (a) and (b) the same? How do they differ? What are they called (the type of relationship between these molecules, not their names).Open the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) and select the Larger Molecules tab. Select an appropriate atoms Kit to build a molecule with two carbon and six hydrogen atoms. Drag atoms into the space above the Kit to make a molecule. A name will appear when you have made an actual molecule that exists (even if it is not the one you want). You can use the scissors tool to separate atoms if you would like to change the connections. Click on 3D to see the molecule, and look at both the space-filling and ball-and-stick possibilities. Draw the structural formula of this molecule and state its name. Can you arrange these atoms in any way to make a different compound? 36. Use the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) to repeat Exercise 2.34, but build a molecule with three carbons, seven hydrogens, and one chlorine. Draw the structural formula of this molecule and slate its name. Can you arrange these atoms to make a different molecule? If so, draw its structural formula and state its name. How are the molecules drawn in (a) and (b) the same? How do they differ? What are they called (the type of relationship between these molecules, not their names)?Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal: uranium bromine strontium neon gold americium rhodium sulfur carbon potassium Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal: cobalt europium iodine indium lithium oxygen cadmium terbium rhenium Using the periodic table, Identify the lightest member of each of the following groups: noble gases alkaline earth metals alkali metals chalcogens Using the periodic table, Identify the heaviest member of each of the following groups: alkali metals chalcogens noble gases alkaline earth metals Use the periodic table to give the name and symbol for each of the following elements: the noble gas in the same period as germanium the alkaline earth metal in the same period as selenium the halogen in the same period as lithium the chalcogen in the same period as cadmium Use the periodic table to give the name and symbol for each of the following elements: the halogen in the same period as the alkali metal with 11 protons the alkaline earth metal in the same period with the neutral noble gas with 18 electrons the noble gas in the same row as an isotope with 30 neutrons and 25 protons the noble gas in the same period as gold Write a symbol for each of the following neutral isotopes. Include the atomic number and mass number for each. the alkali metal with 11 protons and a mass number of 23 the noble gas element with 75 neutrons in its nucleus and 54 electrons in the neutral atom the isotope with 33 protons and 40 neutrons in its nucleus the alkaline earth metal with 88 electrons and 138 neutrons Write a symbol for each of the following neutral isotopes. Include the atomic number and mass number for each. the chalcogen with a mass number of 125 the halogen whose longest-lived isotope is radioactive the noble gas, used in lighting, with 10 electrons and 10 neutrons the lightest alkali metal with three neutrons Using the periodic table, predict whether the following chlorides are ionic or covalent: KCl, NCl3, ICl, MgCl2, PCl5, and CCl4.Using the periodic table, predict whether the following chlorides are ionic or covalent: SiCl4, PCl3, CaCl2, CsCl, CuCl2, and CrCl3.For each of the following compounds, state whether it is ionic or covalent. If it is ionic, write the symbols for the ions involved: NF3 BaO ( NH4)2CO3 Sr(H2 po4)2 IBr Na2O For each of the following compounds, state whether it is ionic or covalent, and if it is ionic, write the symbols for the ions involved: KClO4 Mg(C2H3O2)2 H2S Ag2S N2Cl4 Co( NO3)2 For each of the following pairs of ions, write the formula of the compound they will form: Ca2+,S2 NH4+,SO42 Al3+,Br Na+,HPO42 Mg2+,PO43 For each of the following pairs of ions, write the formula of the compound they will form: K+,O2 NH4+,PO43 Al3+,O2 Na+,O32 Ba2+,PO43 Name the following compounds: CsCl BaO K2S BeCl2 HBr AlF3 AlF3 Name the following compounds: NaF Rb2O BCl3 H2Se P4O6 ICl3 Write the formulas of the following compounds: rubidium bromide magnesium selenide sodium oxide calcium chloride hydrogen fluoride gallium phosphide aluminum bromide ammonium sulfate Write the formulas of the following compounds: lithium carbonate sodium perchlorate barium hydroxide ammonium carbonate sulfuric acid calcium acetate magnesium phosphate sodium sulfite Write the formulas of the following compounds: chlorine dioxide dinitrogen tetraoxide potassium phosphide silver(I) sulfide aluminum nitride silicon dioxide Write the formulas of the following compounds: barium chloride magnesium nitride sulfur dioxide nitrogen trichioride dinitrogen trioxide tin(IV) chloride Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds: Cr2O3 FeCl2 CrO3 TiCl4 CoO MoS2 Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds: (a) NiCO3 (b) MoO3 (c) Co( NO3)2 (d) V2O5 (e) MnO2 (f) Fe2O3 The following ionic compounds are found in common household products. Write the formulas for each compound: potassium phosphate copper(II) sulfate calcium chloride titanium(IV) oxide ammonium nitrate sodium bisulfate (the common name for sodium hydrogen sulfate)The following ionic compounds are found in common household products. Name each of the compounds: Ca(H2 PO4)2 FeSO4 CaCO3 MgO NaNO2 KI What are the IUPAC names of the following compounds? manganese dioxide mercurous chloride ( Hg2Cl2) ferric nitrate [Fe( No 3)3] titanium tetrachioride cupric bromide (CuBr2)What is the total mass (amu) of carbon in each of the following molecules? CH4 CHCl3 C12H12O6 CH3CH2CH2CH2CH3 What is the total mass of hydrogen in each of the molecules? CH4 CHCl3 C12H10O6 CH3CH2CH2CH2CH3 Calculate the molecular or formula mass of each of the following: P4 H2O Ca( NO3)2 CH3CO2H (acetic acid) C12H22O2H11 (sucrose, cane sugar).Determine the molecular mass of the following compounds:Determine the molecular mass of the following compounds:Which molecule has a molecular mass of 28.05 amu?Write a sentence that describes how to determine the number of moles of a compound in a known mass of the compound if we know its molecular formula.Compare 1 mole of H2, 1 mole of O2, and 1 mole of F2. Which has the largest number of molecules? Explain why. Which has the greatest mass? Explain why.Which contains the greatest mass of oxygen: 0.75 mol of ethanol (C2H5OH), 0.60 mol of formic acid (HCO2H), or 1.0 mol of water (H2O)? Explain why.Which contains the greatest number of moles of oxygen atoms: 1 mol of ethanol (C2H5OH), 1 mol of formic acid (HCO2H), or 1 mol of water (H2O)? Explain why.How are the molecular mass and the molar mass of a compound similar and how are they different?Calculate the molar mass of each of the following compounds: hydrogen fluoride, HF ammonia, NH3 nitric acid, HNO3 silver sulfate, Ag2SO4 boric acid, B(OH)3 Calculate the molar mass of each of the following: S8 C5H12 Sc2( SO4)3 CH3COCH3 (acetone) C6H12O6 (glucose)Calculate the empirical or molecular formula mass and the molar mass of each of the following minerals: limestone, CaCO3 halite, NaCl beryl, Be3Al2Si6O18 malachite, Cu2(OH)2CO3 turquoise, CuAl6( PO4)4(OH)8(H2O)4 Calculate the molar mass of each of the following: the anesthetic halothane, C2HBrClF3 the herbicide paraquat, C12H14N2Cl2 caffeine, C8H10N4O2 urea, CO( NH2)2 a typical soap, C17H35CO2Na Determine the number of moles of compound and the number of moles of each type of atom in each of the following: 25.0 g of propylene, C3H6 3.06103 g of the amino acid glycine, C2H5NO2 25 lb of the herbicide Treflan, C13H16N2O4F (1 lb = 454 g) 0.125 kg of the insecticide Paris Green, Cu4(AsO3)2( CH3 CO2)2 325 mg of aspirin, C6H4(CO2H)(CO2CH3)Determine the mass of each of the following: 0.0 146 mol KOH 10.2 mol ethane, C2H6 1.6103 mol Na2 SO4 6.854103 mol glucose, C6 H12O6 2.86 mol Co(NH3)6Cl3 Determine the number of moles of the compound and determine the number of moles of each type of atom in each of the following: 2.12 g of potassium bromide, KBr 0.1488 g of phosphoric acid, H3PO4 23 kg of calcium carbonate, CaCO3 78.452 g of aluminum sulfate, Al2( SO4)3 0.1250 mg of caffeine, C8H10N4O2 Determine the mass of each of the following: 2.345 mol LiCl 0.0872 mol acetylene, C2H2 3.3102 mol Na2CO3 1.23103 mol fructose, C6H12O6 0.5758 mol FeSO4(H2O)7 The approximate minimum daily dietary requirement of the amino acid leucine, C6H13NO2, is 1.1 g. What is this requirement in moles?Determine the mass in grams of each of the following: 0.600 mol of oxygen atoms 0.600 mol of oxygen molecules, O2 0.600 mol of ozone molecules, O3 A 55-kg woman has 7.5103 mol of hemoglobin (molar mass = 64,456 g/mol) in her blood. How many hemoglobin molecules is this? What is this quantity in grams?Determine the number of atoms and the mass of zirconium, silicon, and oxygen found in 0.3384 mol of zircon, ZrSiO4, a semiprecious stone.Determine which of the following contains the greatest mass of hydrogen: 1 mol of CH4, 0.6 mol of C6H6, or 0.4 mol of C3H8.Determine which of the following contains the greatest mass of aluminum: 122 g of AIPO4, 266 g of Al2Cl6, or 225 gof Al2S3.Diamond is one form of elemental carbon. An engagement ring contains a diamond weighing 1.25 carats (1 carat = 200 mg). How many atoms are present in the diamond?The Cullinan diamond was the largest natural diamond ever found (January 25, 1905). It weighed 3104 carats (1 carat = 200 mg). How many carbon atoms were present in the stone?One 55-gram serving of a particular cereal supplies 270 mg of sodium, 11% of the recommended daily allowance. How many moles and atoms of sodium are in the recommended daily allowance?A certain nut crunch cereal contains 11.0 grams of sugar (sucrose, C12H22O11) per serving size of 60.0 grams. How many servings of this cereal must be eaten to consume 0.0278 moles of sugar?A tube of toothpaste contains 0.76 g of sodium monofluorophosphate (Na2PO3F) in 100 mL. What mass of fluorine atoms in mg was present? How many fluorine atoms were present?Which of the following represents the least number of molecules? 20.0 g of H2O (18.02 glmol) 77.0 g of CH4 (16.06 glmol) 68.0 g of CaH2 (42.09 g/mol) 100.0 g of N2O (44.02 g/mol) 840 g of HF (20.01 g/mol)What information do we need to determine the molecular formula of a compound from the empirical formula?Calculate the following to four significant figures: the percent composition of ammonia, NH3 the percent composition of photographic fixer solution (hypo), Na2S2O3 the percent of calcium ion in Ca3(PO4)2 Determine the following to four significant figures: the percent composition of hydrazoic acid, HN3 the percent composition of TNT,C6H2(CH3)( NO2)3 the percent of SO42 in Al2( SO4)3 Determine the percent ammonia, NH3, in Co( NH3)6Cl3, to three significant figures.Determine the percent water in CuSO45H2O to three significant figures.Determine the empirical formulas for compounds with the following percent compositions: 15.8% carbon and 84.2% sulfur 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen Determine the empirical formulas for compounds with the following percent compositions: 43.6% phosphorus and 56.4% oxygen 28.7% K, 1.5% H, 22.8% P, and 47.0% O A compound of carbon and hydrogen contains 92.3% C and has a molar mass of 78.1 g/mol. What is its molecular formula?Dichioroethane, a compound that is often used for dry cleaning, contains carbon, hydrogen, and chlorine. It has a molar mass of 99 g/mol. Analysis of a sample shows that it contains 24.3% carbon and 4.1% hydrogen. What is its molecular formula?Determine the empirical and molecular formula for chrysotile asbestos. Chrysotile has the following percent composition: 28.03% Mg, 21.60% Si, 1.16% H, and 49.21% O. The molar mass for chrysotile is 520.8 g/mol.Polymers are large molecules composed of simple units repeated many times. Thus, they often have relatively simple empirical formulas. Calculate the empirical formulas of the following polymers: Lucite (Plexiglas); 59.9% C, 8.06% H, 32.0% O Saran; 24.8% C, 2.0% H, 73.1% C1 polyethylene; 86% C, 14% H polystyrene; 92.3% C, 7.7% H Orlon; 67.9% C, 5.70% H, 26.4% N A major textile dye manufacturer developed a new yellow dye. The dye has a percent composition of 75.95% C, 17.72% N, and 6.33% H by mass with a molar mass of about 240 g/mol. Determine the molecular formula of the dye.Explain what changes and what stays the same when 1.00 L of a solution of NaCl is diluted to 1.80 L.What information do we need to calculate the molarity of a sulfuric acid solution?What does it mean when we say that a 200-mL sample and a 400-mL sample of a solution of salt have the same molarity? In what ways are the two samples identical? In what ways are these two samples different?Determine the molarity for each of the following solutions: (a) 0.444 mol of CoCl2 in 0.654 L of solution (b) 98.0 g of phosphoric acid, H3PO4, in 1.00 L of solution (c) 0.2074 g of calcium hydroxide, Ca(OH)2, in 40.00 mL of solution (d) 10.5 kg of Na2SO410H2O in 18.60 L of solution (e) 7.0103 mol of I2 in 100.0 mL of solution (f) 1.8104 mg of HCI in 0.075 L of solution Determine the molarity of each of the following solutions: (a) 1.457 mol KCl in 1.500 L of solution (b) 0.515 g of H2SO4 in 1.00 L of solution (c) 20.54 g of Al( NO3)3 in 1575 mL of solution (d) 2.76 kg of CuSO45H2O in 1.45 L of solution (e) 0.005653 mol of Br2 in 10.00 mL of solution (f) 0.000889 g of glycine, C2H5NO2, in 1.05 mL of solution Consider this question: What is the mass of the solute in 0.500 L of 0.30 M glucose, C6H12O6, used for intravenous injection? (a) Outline the steps necessary to answer the question. (b) Answer the question.Consider this question: What is the mass of solute in 200.0 L of a 1.556-M solution of KBr? (a) Outline the steps necessary to answer the question. (b) Answer the question.Calculate the number of moles and the mass of the solute in each of the following solutions: (a) 2.00 L of 18.5MH2SO4, concentrated sulfuric acid (b) 100.0 mL of 3.8105MNaCN, the minimum lethal concentration of sodium cyanide in blood serum (c) 5.50 L of 13.3 MH2CO, the formaldehyde used to fix tissue samples (d) 325 mL of 1.8106MFeSO4, the minimum concentration of iron sulfate detectable by taste in drinking water Calculate the number of moles and the mass of the solute in each of the following solutions: (a) 325 mL of 8.23105M KI, a source of iodine in the diet (b) 75.0 mL of 2.2105MH2SO4, a sample of acid rain (c) 0.2500 L of 0.1135 MK2CrO4, an analytical reagent used in iron assays (d) 10.5 L of 3.7 16 M( NH4)2SO4, a liquid fertilizer Consider this question: What is the molarity of KMnO4 in a solution of 0.0908 g of KMnO4 in 0.500 L of solution? (a) Outline the steps necessary to answer the question. (b) Answer the question.Consider this question: What is the molarity of HCl if 35.23 mL of a solution of HCl contain 0.3366 g of HCl? (a) Outline the steps necessary to answer the question. (b) Answer the question.Calculate the molarity of each of the following solutions: (a) 0.195 g of cholesterol, C27H46O, in 0.100 L of serum, the average concentration of cholesterol in human serum (b) 4.25 g of NH3 in 0.500 L of solution, the concentration of NH3 in household ammonia (c) 1.49 kg of isopropyl alcohol, C3H7OH, in 2.50 L of solution, the concentration of isopropyl alcohol in rubbing alcohol (d) 0.029 g of I2 in 0.100 L of solution, the solubility of I2 in water at 20 C Calculate the molarity of each of the following solutions: (a) 293 g HCl in 666 mL of solution, a concentrated HCl solution (b) 2.026 g FeCl3 in 0.1250 L of a solution used as an unknown in general chemistry laboratories (c) 0.00 1 mg Cd2+ in 0.100 L, the maximum permissible concentration of cadmium in drinking water (d) 0.0079 g C7H5SNO3 in one ounce (29.6 mL), the concentration of saccharin in a diet soft drink.There is about 1.0 g of calcium, as Ca2+, in LO L of milk. What is the molarity of Ca2+ in milk?What volume of a 1.00MFe( NO3)3 solution can be diluted to prepare 1.00 L of a solution with a concentration of 0.250 M?If 0.1718 L of a 0.3556-M C3H7OH solution is diluted to a concentration of 0.1222 M, what is the volume of the resulting solution?If 4.12 L of a 0.850 MH3PO4 solution is be diluted to a volume of 10.00 L, what is the concentration of the resulting solution?What volume of a 0.33MC12H22O11 solution can be diluted to prepare 25 mL of a solution with a concentration of 0.025 M?What is the concentration of the NaCl solution that results when 0.150 L of a 0.556-M solution is allowed to evaporate until the volume is reduced to 0.105 L?What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume? (a) 1.00 L of a 0.250-M solution of Fe( NO3)3 is diluted to a final volume of 2.00 L (b) 0.5000 L of a 0.1222-M solution of C3H7OH is diluted to a final volume of 1.250 L (c) 2.35 L of a 0.350-M solution of H3PO is diluted to a final volume of 4.00 L (d) 22.50 mL of a 0.025-M solution of C12H22O11 is diluted to 100.0 mL What is the final concentration of the solution produced when 225.5 mL of a 0.09988-M solution of Na2CO3 is allowed to evaporate until the solution volume is reduced to 45.00 mL?A 2.00-L bottle of a solution of concentrated HCl was purchased for the general chemistry laboratory. The solution contained 868.8 g of HCl. What is the molarity of the solution?An experiment in a general chemistry laboratory calls for a 2.00-M solution of HCl. How many mL of 11.9 M HCl would be required to make 250 mL of 2.00 M HCl?What volume of a 0.20MK2SO4 solution contains 57 g of K2SO4?The US Environmental Protection Agency (EPA) places limits on the quantities of toxic substances that may be discharged into the sewer system. Limits have been established for a variety of substances, including hexavalent chromium, which is limited to 0.50 mg/L. If an industry is discharging hexavalent chromium as potassium dichromate (K2Cr2O7), what is the maximum permissible molarity of that substance?Consider this question: What mass of a concentrated solution of nitric acid (68.0% HNO3 by mass) is needed to prepare 400.0 g of a 10.0% solution of HNO3 by mass? (a) Outline the steps necessary to answer the question. (b) Answer the question.What mass of a 4.00% NaOH solution by mass contains 15.0 g of NaOH?What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3, which is equivalent to milligrams of CaCO3 per liter of water. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175 mg CaCO3/L?The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3, which is equivalent to milligrams of CaCO3 per liter of water. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175 mg CaCO3/L?In Canada and the United Kingdom, devices that measure blood glucose levels provide a reading in millimoles per liter. If a measurement of 5.3 mM is observed, what is the concentration of glucose (C6H12O6) in mg/dL?A throat spray is 1.40% by mass phenol, C6H5OH, in water. If the solution has a density of 0.9956 g/mL, calculate the molarity of the solution.Copper(I) iodide (CuI) is often added to table salt as a dietary source of iodine. How many moles of CuI Are contained in 1.00 lb (454 g) of table salt containing 0.0100% CuI by mass?A cough syrup contains 5.0% ethyl alcohol, C2H5OH, by mass. If the density of the solution is 0.9928 g/mL, determine the molarity of the alcohol in the cough syrup.D5W is a solution used as an intravenous fluid. It is a 5.0% by mass solution of dextrose (C6H12O6) in water. If the density of D5W is 1.029 g/mL, calculate the molarity of dextrose in the solution.Find the molarity of a 40.0% by mass aqueous solution of sulfuric acid, H2SO4, for which the density is 1.3057 g/mL.What does it mean to say an equation is balanced? Why is it important for an equation to be balanced?Consider molecular, complete ionic, and net ionic equations. (a) What is the difference between these types of equations? (b) In what circumstance would the complete and net ionic equations for a reaction be identical?Balance the following equations: (a) PCl5(s)+H2O(l)POCl3(l)+HCl(aq) (b) Cu(s)+HNO3(aq)Cu( NO3)2(aq)+H2O(l)+NO(g) (c) H2(g)+I2(s)HI(s) (d) Fe(s)+O2(g)Fe2O3(s) (e) Na(s)+H2O(l)NaOH(aq)+H2(g) (f) ( NH4)2Cr2O7(s)Cr2O3(s)+N2(g)+H2O(g) (g) P4(s)+Cl2(g)PCl3(l) (h) PtCl4(s)Pt(s)+Cl2(g)Balance the following equations: (a) Ag(s)+H2S(g)+O2(g)Ag2S(s)+H2O(l) (b) P4(s)+O2(g)P4O10(s) (c) Pb(s)+H2O(l)+O2(g)Pb(OH)2(s) (d) Fe(s)+H2O(l)Fe3O4(s)+H2(g) (e) Sc2O2(s)+SO3(l)Sc2( SO4)3(s) (f) Ca( PO4)2(aq)+H3PO4(aq)Ca(H2 PO4)2(aq) (g) Al(s)+H2SO4(aq)Al2( SO4)3(s)+H2(g) (h) TiCl4(s)+H2O(g)TiO2(s)+HCl(g)Write a balanced molecular equation describing each of the following chemical reactions. (a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas. (b) Gaseous butane, C4H10, reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor. (c) Aqueous solutions of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride. (d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.Write a balanced equation describing each of the following chemical reactions. (a) Solid potassium chlorate, KClO3, decomposes to form solid potassium chloride and diatomic oxygen gas. (b) Solid aluminum metal reacts with solid diatomic iodine to form solid Al2I6. (c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced. (d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.Colorful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of the metals magnesium, aluminum, and iron with oxygen. (a) Write the formulas of barium nitrate and potassium chlorate. (b) The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction. (c) The decomposition of solid barium nitrate leads to the formation of solid barium oxide, diatomic nitrogen gas, and diatomic oxygen gas. Write an equation for the reaction. (d) Write separate equations for the reactions of the solid metals magnesium, aluminum, and iron with diatomic oxygen gas to yield the corresponding metal oxides. (Assume the iron oxide contains Fe3+ ions.)Fill in the blank with a single chemical formula for a covalent compound that will balance the equation:Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide). (a) Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water. (b) The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solutions of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process. (a) The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide. (b) The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water. (c) Solid calcium hydroxide is then added to the seawater, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride. (d) The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water. (e) Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.From the balanced molecular equations, write the complete ionic and net ionic equations for the following: (a) K2C2O4(aq)+Ba(OH)2(aq)2HOH(aq)+BaC2O4(s) (b) Pb( NO3)2(aq)+H2SO4(aq)PbSO4(s)+2HNO3(aq) (c) CaCO3(s)+H2SO4(aq)CaSO4(s)+CO2(g)+H2O(l)Use the following equations to answer the next four questions: H2O(s)H2O(l) Na+(aq)+Cl(aq)+Ag+(aq)+NO3(aq)AgCl(s)+Na+(aq)+NO3(aq) CH3OH(g)+O2(g)CO2(g)+H2O(g) 2H2O(l)2H2(g)+O2(g) H+(aq)+OH(aq)H2O(l) (a) Which equation describes a physical change? (b) Which equation identifies the reactants and products of a combustion reaction? (c) Which equation is not balanced? (d) Which is a net ionic equation?Indicate what type, or types, of reaction each of the following represents: (a) Ca(s)+Br2(l)CaBr2(s) (b) Ca(OH)2(aq)+2HBr(aq)CaBr2(aq)+2H2O(l) (c) C6H12(l)+9O2(g)6CO2(g)+6H2O(g)Indicate what type, or types, of reaction each of the following represents: (a) H2O(g)+C(s)CO(g)+H2(g) (b) 2KClO3(s)2KCl(s)+3O2(g) (c) Al(OH)3(aq)+3HCl(aq)AlCl3(aq)+3H2O(l) (d) Pb( NO3)2(aq)+H2SO4(aq)PbSO4(s)+2HNO3(aq)Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.Determine the oxidation states of the elements in the following compounds: (a) Nal (b) GdCl3 (c) LiNO3 (d) H2Se (e) Mg2Si (f) RbO2, rubidium superoxide (g) HF Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides. (a) H3PO4 (b) Al(OH)3 (c) SeO2 (d) KNO2 (e) ln2S3 (f) P4O6 Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides. (a) H2SO4 (b) Ca(OH)2 (C) BrOH (d) ClNO2 (e) TiCl4 (f) NaH Classify the following as acid-base reactions or oxidation-reduction reactions: (a) Na2S(aq)+2HCl(aq)2NaCl(aq)+H2(g) (b) 2Na(s)+2HCl(aq)2NaCl(aq)+H2(g) (c) Mg(s)+Cl2(g)MgCl2(s) (d) MgO(s)+2HCl(aq)MgCl2(aq)+H2+O(l) (e) K3P(s)+2O2(g)K3PO4(s) (f) 2KOH(aq)+H3PO4(aq)K3PO4(aq)+3H2O(l)Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations: (a) Mg(s)+NiCl2(aq)MgCl2(aq)+Ni(s) (b) PCl3(l)+Cl2(g)PCl5(s) (c) C2H4(g)+3O2(g)2CO2(g)+2H2O(g) (d) Zn(s)+H2SO4(aq)ZnSO4(aq)+H2(g) (e) 2K2S2O3(s)+I2(s)K2S4O6(s)+2KI(s) (f) 3Cu(s)+8HNO3(aq)3Cu( NO3)2(aq)+2NO(g)+4H2O(l)Complete and balance the following acid-base equations: (a) HCl gas reacts with solid Ca(OH)2(s). (b) A solution of Sr(OH)2 is added to a solution of HNO3.Complete and balance the following acid-base equations: (a) A solution of HClO4 is added to a solution of LiOH. (b) Aqueous H2SO4 reacts with NaOH. (c) Ba(OH)2 reacts with HF gas.Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. (a) Al(s)+F2(g) (b) Al(s)+CuBr2(aq) (single displacement) (c) P4(s)+O2(g) (d) Ca(s)+H2O(l) (products are a strong base and a diatomic gas)Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. (a) K(s)+H2O(l) (b) Ba(s)+HBr(aq) (c) Sn(s)+I2(s)Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used. (a) Mg(OH)2(s)+HCl4(aq) (b) SO3(g)+H2O(l) (assume an excess of water and that the product dissolves) (c) SrO(s)+H2SO4(l)When heated to 700—800 C, diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They burn!) Write the balanced equation for this reaction.The military has experimented with lasers that produce very intense light when fluorine combines explosively with hydrogen. What is the balanced equation for this reaction?Write the molecular, total ionic, and net ionic equations for the following reactions: (a) Ca(OH)2(aq)+HC2H3O2(aq) (b) H3PO4(aq)+CaCl2(aq)Great Lakes Chemical Company produces bromine, Br2, from bromide salts such as NaBr, in Arkansas brine by treating the brine with chlorine gas. Write a balanced equation for the reaction of NaBr with Cl2.In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Write an equation for the reaction that involves 2 mol of LiOH per 1 mol of CO2. (Hint: Water is one of the products.)Calcium propionate is sometimes added to bread to retard spoilage. This compound can be prepared by the reaction of calcium carbonate, CaCO3, with propionic acid, C2H5CO2H, which has properties similar to those of acetic acid. Write the balanced equation for the formation of calcium propionate.Complete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas: (a) Ca(OH)2(s)+H2S(g) (b) Na2CO3(aq)+H2S(g)Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required. (a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid) (b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction (c) gaseous H2S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid)Calcium cyclamate Ca(C6H 11 NHSO3)2 is an artificial sweetener used in many countries around the world but is banned in the United States. It can be purified industrially by converting it to the barium salt through reaction of the acid C6H11NHSO3H with barium carbonate, treatment with sulfuric acid (barium sulfate is very insoluble), and then neutralization with calcium hydroxide. Write the balanced equations for these reactions.Complete and balance each of the following half-reactions (steps 2—5 in half-reaction method): (a) Sn4+(aq)Sn2+(aq) (b) [Ag( NH 3)2]+(aq)Ag(s)+NH3(aq) (c) Hg2Cl2(s)Hg(l)+Cl(aq) (d) H2O(l)O2(g) (in acidic solution) (e) IO3(aq)I2(s) (f) SO32(aq)SO42(aq) (in acidic solution) (g) MnO4(aq)Mn2+(aq) (in acidic solution) (h) CI(aq)CIO3(aq) (in basic solution)Complete and balance each of the following half-reactions (steps 25 in half-reaction method): (a) Cr2+(aq)Cr3+(aq) (b) Hg(l)+Br(aq)HgBr42(aq) (c) ZnS(s)Zn(s)+S2(aq) (d) H2(g)H2O(l) (in basic solution) (e) H2(g)H3O+(aq) (in acidic solution) (f) NO3(aq)HNO2(aq) (in acidic solution) (g) MnO2(s)MnO4(aq) (in basic solution) (h) Cl(aq)ClO3(aq) (in acidic solution)Balance each of the following equations according to the half-reaction method: (a) Sn2+(aq)+Cu2+(aq)S4+(aq)+Cu+(aq) (b) H2S(g)+Hg22+(aq)Hg(l)+S(s)(inacid) (c) CN(aq)+ClO2(aq)CNO(aq)+Cl(aq)(inacid) (d) Fe2+(aq)+Ce4+(aq)Fe3+(aq)+Ce3+(aq) (e) HBrO(aq)Br(aq)+O2(g)(inacid)Balance each of the following equations according to the half-reaction method: (a) Zn(s)+NO3(aq)Zn2+(aq)+N2(g)(inacid) (b) Zn(s)+NO3(aq)Zn2+(aq)+NH2(aq)(inbase) (c) CuS(s)+NO3(aq)Cu2+(aq)+S(s)+NO(g)(inacid) (d) NH2(g)+O2(g)NO2(g)(gasephase) (e) Cl2(g)+OH(aq)Cl1(aq)+Cl3(aq)(inbase) (f) H2O2(aq)+MnO4(aq)Mn2+(aq)+O2(g)(inacid) (g) NO2(g)NO3(aq)+NO2(aq)(inbase) (h) Fe3+(aq)+I(aq)Fe2+(aq)+I2(aq)Balance each of the following equations according to the half-reaction method: (a) MnO4(aq)+NO2(aq)MnO2(s)+NO3(aq) (in base) (b) MnO42(aq)MnO42(aq)+MnO2(s) (in base) (c) Br2(l)+SO2(g)Br(aq)+SO42(aq) (in acid)Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following: (a) The number of moles and the mass of chlorine, Cl2, required to react with 10.0 g of sodium metal, Na, to produce sodium chloride, NaCl. (b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide. (c) The number of moles and the mass of sodium nitrate, NaNO3, required to produce 128 g of oxygen. ( NaNO2 is the other product.) (d) The number of moles and the mass of carbon dioxide formed by the combustion of 20.0 kg of carbon in an excess of oxygen. (e) The number of moles and the mass of copper(II) carbonate needed to produce 1.500 kg of copper(II) oxide. ( CO2 is the other product.) (f) The number of moles and the mass of formed by the reaction of 12.85 g of with an excess of Br2.Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following: (a) The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2. (b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide. (c) The number of moles and the mass of magnesium carbonate, MgCO3, required to produce 283 g of carbon dioxide. (MgO is the other product.) (d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen. (e) The number of moles and the mass of barium peroxide, BaO2, needed to produce 2.500 kg of barium oxide, BaO ( O2 is the other product.) (f) The number of moles and the mass of required to react with H2O to produce 9.55 g of 43. Determine the number of moles and the mass requested for each reaction in Exercise 4.42.Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following: (a) The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2. (b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide. (c) The number of moles and the mass of magnesium carbonate, MgCO3, required to produce 283 g of carbon dioxide. (MgO is the other product.) (d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen. (e) The number of moles and the mass of barium peroxide, BaO2, needed to produce 2.500 kg of barium oxide, BaO ( O2 is the other product.) (f) The number of moles and the mass of required to react with H2O to produce 9.55 g of Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following: (a) The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2. (b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide. (c) The number of moles and the mass of magnesium carbonate, MgCO3, required to produce 283 g of carbon dioxide. (MgO is the other product.) (d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen. (e) The number of moles and the mass of barium peroxide, BaO2, needed to produce 2.500 kg of barium oxide, BaO ( O2 is the other product.) (f) The number of moles and the mass of required to react with H2O to produce 9.55 g of 45. Determine the number of moles and the mass requested for each reaction in Exercise 4.44.H2 is produced by the reaction of 118.5 mL of a 0.8775-M solution of H3PO4 according to the following equation: 2Cr+2H3PO43H2+2CrPO4. (a) Outline the steps necessary to determine the number of moles and mass of H2. (b) Perform the calculations outlined.Gallium chloride is formed by the reaction of 2.6 L of a 1.44 M solution of HCl according to the following equation: 2Ga+6HCl2GaCl3+3H2. (a) Outline the steps necessary to determine the number of moles and mass of gallium chloride. (b) Perform the calculations outlined.I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation: 2CuCl2+4KICuCl+4KCl+I2 (a) How many molecules of I2 are produced? (b) What mass of I2 is produced?Silver is often extracted from ores such as K[Ag(CN)2] and then recovered by the reaction 2K[Ag(CN)2](aq)+Zn(s)2Ag(s)+Zn(CN)2(aq)+2KCN(aq) (a) How many molecules of Zn(CN)2 are produced by the reaction of 35.27 g of K[Ag(CN)2]? (b) What mass of Zn(CN)2 is produced?What mass of silver oxide, Ag2O, is required to produce 25.0 g of silver sulfadiazine, AgC10H9N4SO2, from the reaction of silver oxide and sulfadiazine? 2C10H10N4SO2+Ag2O2AgC10H9N4SO2+H2O Carborundum is silicon carbide, SiC, a very hard material used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO2, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. Write the balanced equation for the reaction, and calculate how much SiO2 is required to produce 3.00 kg of SiC.Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed. 2NaN3(s)2Na(s)+3N2(g) What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?Urea, CO( NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO2 produced by combustion of 1.00103 kg of carbon followed by the reaction? CO2(g)+2NH3(g)CO( NH2)2(s)+H2O(l)In an accident, a solution containing 2.5 kg of nitric acid was spilled. Two kilograms of Na2CO3 was quickly spread on the area and CO2 was released by the reaction. Was sufficient Na2CO3 used to neutralize all of the acid?A compact car gets 37.5 miles per gallon on the highway. If gasoline contains 84.2% carbon by mass and has a density of 0.8205 g/mL, determine the mass of carbon dioxide produced during a 500-mile trip (3.785 liters per gallon).What volume of 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s)+H2SO4(l)HCl(g)+NaHSO4(s)What volume of a 0.2089 M Kl solution contains enough KI to react exactly with the Cu( NO3)2 in 43.88 mL of a 0.3842 M solution of Cu( NO3)2? 2Cu( NO3)2+4KI2CuI+I2+4KNO3 A mordant is a substance that combines with a dye to produce a stable fixed color in a dyed fabric. Calcium acetate is used as a mordant. It is prepared by the reaction of acetic acid with calcium hydroxide. 2CH3CO2H+Ca(OH)2Ca( CH3 CO2)2+2H2O What mass of Ca(OH)2 is required to react with the acetic acid in 25.0 mL of a solution having a density of 1.065 g/mL and containing 58.0% acetic acid by mass?The toxic pigment called white lead, Pb3(OH)2( CO3)2, has been replaced in white paints by rutile, TiO2. How much rutile (g) can be prepared from 379 g of an ore that contains 88.3% ilmenite (FeTiO3) by mass? 2FeTiO3+4HCl+Cl22FeCl3+2TiO2+2H2O The following quantities are placed in a container: 1.51024 atoms of hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen. What is the total mass in grams for the collection of all three elements? What is the total number of moles of atoms for the three elements? If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, one sulfur atom, and four oxygen atoms, which substance is consumed first? How many atoms of each remaining element would remain unreacted in the change described in (c)?

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