Bundle: General Chemistry, Loose-leaf V...11th EditionDarrell Ebbing, Steven D. Gammon Publisher: Cengage LearningISBN: 9781337128391
Bundle: General Chemistry, Loose-leaf V...
Solutions for Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2, 4 terms (24 months) Printed Access Card
Problem 1.1QP:
Discuss some ways in which chemistry has changed technology. Give one or more examples of how...Problem 1.2QP:
Define the terms experiment and theory. How are theory and experiment related? What is a hypothesis?Problem 1.3QP:
Illustrate the steps in the scientific method using Rosenbergs discovery of the anticancer activity...Problem 1.9QP:
Give examples of an element, a compound, a heterogeneous mixture, and a homogeneous mixture.Problem 1.10QP:
What phases or states of matter are present in a glass of bubbling carbonated beverage that contains...Problem 1.15QP:
How does the International System (SI) obtain units of different size from a given unit? How does...Problem 1.18QP:
Why should units be carried along with numbers in a calculation?Problem 1.19QP:
When the quantity 12.9 g is added to 2 1002 g, how many significant figures should be reported in...Problem 1.21QP:
A 75.0-g sample of a pure liquid, liquid A, with a density of 3.00 g/mL is mixed with a 50.0-mL...Problem 1.22QP:
Which of the following represents the smallest mass? a 23 cg b 2.3 103 g c 0.23 mg d 0.23 g e 2.3 ...Problem 1.23QP:
Physical and Chemical Changes Say you are presented with two beakers, beaker A and beaker B, each...Problem 1.25QP:
a Sodium metal is partially melted. What are the two phases present? b A sample of sand is composed...Problem 1.26QP:
A material is believed to be a compound. Suppose you have several samples of this material obtained...Problem 1.27QP:
You need a thermometer that is accurate to 5C to conduct some experiments in the temperature range...Problem 1.28QP:
Imagine that you get the chance to shoot five arrows at each of the targets depicted below. On each...Problem 1.29QP:
Say you live in a climate where the temperature ranges from 100F to 20F and you want to define a new...Problem 1.30QP:
You are presented with a piece of metal in a jar. It is your job to determine what the metal is....Problem 1.31QP:
You have two identical boxes with interior dimensions of 8.0 cm 8.0 cm 8.0 cm. You completely fill...Problem 1.32QP:
Consider the following compounds and their densities. You create a column of the liquids in a glass...Problem 1.33QP:
Which of the following items have a mass of about 1 g? a grain of sand a paper clip a nickel a...Problem 1.34QP:
What is the length of the nail reported to the correct number of significant figures?Problem 1.35QP:
For these questions, be sure to apply the rules for significant figures. a You are conducting an...Problem 1.36QP:
You are teaching a class of second graders some chemistry, and they are confused about an objects...Problem 1.37QP:
A 15.5 g sample of sodium carbonate is added to a solution of acetic acid weighing 19.7 g. The two...Problem 1.38QP:
Some iron wire weighing 5.6 g is placed in a beaker and covered with 15.0 g of dilute hydrochloric...Problem 1.39QP:
Zinc metal reacts with yellow crystals of sulfur in a fiery reaction to produce a white powder of...Problem 1.40QP:
Aluminum metal reacts with bromine, a red-brown liquid with a noxious odor. The reaction is vigorous...Problem 1.41QP:
Give the normal state (solid, liquid, or gas) of each of the following. a sodium hydrogen carbonate...Problem 1.42QP:
Give the normal state (solid, liquid, or gas) of each of the following. a potassium hydrogen...Problem 1.43QP:
Which of the following are physical changes and which are chemical changes? a melting of sodium...Problem 1.44QP:
For each of the following, decide whether a physical or a chemical change is involved. a dissolving...Problem 1.45QP:
A sample of mercury(II) oxide was heated to produce mercury metal and oxygen gas. Then the liquid...Problem 1.46QP:
Solid iodine, contaminated with salt, was heated until the iodine vaporized. The violet vapor of...Problem 1.47QP:
The following are properties of substances. Decide whether each is a physical property or a chemical...Problem 1.48QP:
Decide whether each of the following is a physical property or a chemical property of the substance....Problem 1.49QP:
Iodine is a solid having somewhat lustrous, blue-black crystals. The crystals vaporize readily to a...Problem 1.50QP:
Mercury(II) oxide is an orange-red solid with a density of 11.1 g/cm3. It decomposes when heated to...Problem 1.51QP:
Consider the following separations of materials. State whether a physical process or a chemical...Problem 1.52QP:
All of the following processes involve a separation of either a mixture into substances or a...Problem 1.53QP:
Label each of the following as a substance, a heterogeneous mixture, or a solution. a seawater b...Problem 1.54QP:
Indicate whether each of the following materials is a substance, a heterogeneous mixture, or a...Problem 1.55QP:
Which of the following are pure substances and which are mixtures? For each, list all of the...Problem 1.56QP:
Which of the following are pure substances and which are mixtures? For each, list all of the...Problem 1.57QP:
How many significant figures are there in each of the following measurements? a 57.00 g b 0.0503 kg...Problem 1.58QP:
How many significant figures are there in each of the following measurements? a 4.0100 mg b 0.05930...Problem 1.59QP:
The circumference of the earth at the equator is 40,000 km. This value is precise to two significant...Problem 1.60QP:
The astronomical unit equals the mean distance between the earth and the sun. This distance is...Problem 1.61QP:
Assuming all numbers are measured quantities, do the indicated arithmetic and give the answer to the...Problem 1.62QP:
Assuming all numbers are measured quantities, do the indicated arithmetic and give the answer to the...Problem 1.65QP:
Write the following measurements, without scientific notation, using the appropriate SI prefix. a...Problem 1.66QP:
Write the following measurements, without scientific notation, using the appropriate SI prefix. a...Problem 1.67QP:
Using scientific notation, convert: a 6.15 ps to s b 3.781 m to m c 1.546 to m d 9.7 mg to gProblem 1.68QP:
Using scientific notation, convert: a 6.20 km to m b 1.98 ns to s c 2.54 cm to m d 5.23 g to gProblem 1.69QP:
Convert: a 68F to degrees Celsius b 23F to degrees Celsius c 26C to degrees Fahrenheit d 81C to...Problem 1.70QP:
Convert: a 51F to degrees Celsius b 11F to degrees Celsius c 41C to degrees Fahrenheit d 22C to...Problem 1.71QP:
Salt and ice are stirred together to give a mixture to freeze ice cream. The temperature of the...Problem 1.73QP:
A certain sample of the mineral galena (lead sulfide) weighs 12.4 g and has a volume of 1.64 cm3....Problem 1.74QP:
A flask contains a 30.0 mL sample of acetone (nail polish remover) that weighs 23.6 grams. What is...Problem 1.75QP:
A liquid with a volume of 8.5 mL has a mass of 6.71 g. The liquid is either octane, ethanol, or...Problem 1.78QP:
What is the mass of a 43.8-mL sample of gasoline, which has a density of 0.70 g/cm3?Problem 1.79QP:
Ethanol has a density of 0.789 g/cm3. What volume must be poured into a graduated cylinder to give...Problem 1.80QP:
Bromine is a red-brown liquid with a density of 3.10 g/mL. A sample of bromine weighing 88.5 g...Problem 1.81QP:
Sodium hydrogen carbonate, known commercially as baking soda, reacts with acidic materials such as...Problem 1.82QP:
The acidic constituent in vinegar is acetic acid. A 10.0-mL sample of a certain vinegar contains 611...Problem 1.83QP:
The different colors of light have different wavelengths. The human eye is most sensitive to light...Problem 1.84QP:
Water consists of molecules (groups of atoms). A water molecule has two hydrogen atoms, each...Problem 1.85QP:
The total amount of fresh water on earth is estimated to be 3.73 108 km3. What is this volume in...Problem 1.86QP:
A submicroscopic particle suspended in a solution has a volume of 1.3 m3. What is this volume in...Problem 1.87QP:
How many grams are there in 3.58 short tons? Note that 1 g = 0.03527 oz (ounces avoirdupois), 1 lb...Problem 1.89QP:
The first measurement of sea depth was made in 1840 in the central South Atlantic, where a plummet...Problem 1.90QP:
The estimated amount of recoverable oil from the field at Prudhoc Bay in Alaska is 1.3 1010...Problem 1.91QP:
A fish tank is 24.2 in. long, 15.9 in. deep, and 14.8 in. high. What is the maximum volume of water,...Problem 1.92QP:
The population density of worms in a particular field is 33 worms per cubic meter of soil. How many...Problem 1.94QP:
An antacid tablet weighing 0.853 g contained calcium carbonate as the active ingredient, in addition...Problem 1.95QP:
When a mixture of aluminum powder and iron(III) oxide is ignited, it produces molten iron and...Problem 1.96QP:
When chlorine gas is bubbled into a solution of sodium bromide, the sodium bromide reacts to give...Problem 1.97QP:
A beaker weighed 50.90 g. To the beaker was added 5.680 g of iron pellets and 53.3 g of hydrochloric...Problem 1.99QP:
Describe each of the following as a physical or chemical property of each listed chemical substance....Problem 1.100QP:
Describe each of the following as a physical or chemical property of each listed chemical substance....Problem 1.101QP:
Analyses of several samples of a material containing only iron and oxygen gave the following...Problem 1.102QP:
A red-orange solid contains only mercury and oxygen. Analyses of three different samples gave the...Problem 1.103QP:
A cubic box measures 39.3 cm on an edge. What is the volume of the box in cubic centimeters? Express...Problem 1.104QP:
A cylinder with circular cross section has a radius of 2.56 cm and a height of 56.32 cm. What is the...Problem 1.105QP:
An aquarium has a rectangular cross section that is 47.8 in. by 12.5 in.; it is 19.5 in. high. How...Problem 1.106QP:
A spherical tank has a radius of 175.0 in. Calculate the volume of the tank in cubic inches; then...Problem 1.107QP:
Obtain the difference in volume between two spheres, one of radius 5.61 cm, the other of radius 5.85...Problem 1.108QP:
What is the difference in surface area between two circles, one of radius 7.98 cm, the other of...Problem 1.109QP:
Perform the following arithmetic setups and express the answers to the correct number of significant...Problem 1.111QP:
For each of the following, write the measurement in terms of an appropriate prefix and base unit. a...Problem 1.112QP:
For each of the following, write the measurement in terms of an appropriate prefix and base unit. a...Problem 1.113QP:
Write each of the following in terms of the SI base unit (that is, express the prefix as the power...Problem 1.114QP:
Write each of the following in terms of the SI base unit (that is, express the prefix as the power...Problem 1.115QP:
Tungsten metal, which is used in lightbulb filaments, has the highest melting point of any metal...Problem 1.116QP:
Titanium metal is used in aerospace alloys to add strength and corrosion resistance. Titanium melts...Problem 1.117QP:
Calcium carbonate, a white powder used in toothpastes, antacids, and other preparations, decomposes...Problem 1.119QP:
Gallium metal can be melted by the heat of ones hand. Its melting point is 29.8C. What is this...Problem 1.120QP:
Mercury metal is liquid at normal temperatures but freezes at 38.9C. What is this temperature in...Problem 1.121QP:
Zinc metal can be purified by distillation (transforming the liquid metal to vapor, then condensing...Problem 1.122QP:
Iodine is a bluish-black solid. It forms a violet-colored vapor when heated. The solid melts at...Problem 1.123QP:
An aluminum alloy used in the construction of aircraft wings has a density of 2.70 g/cm3. Express...Problem 1.124QP:
Vanadium metal is added to steel to impart strength. The density of vanadium is 5.96 g/cm3. Express...Problem 1.125QP:
The density of quartz mineral was determined by adding a weighed piece to a graduated cylinder...Problem 1.127QP:
Some bottles of colorless liquids were being labeled when the technicians accidentally mixed them up...Problem 1.128QP:
Providing no reaction occurs, a solid will float on any liquid that is more dense than it is. The...Problem 1.129QP:
Platinum metal is used in jewelry; it is also used in automobile catalytic converters. What is the...Problem 1.130QP:
Ultrapure silicon is used to make solid-state devices, such as computer chips. What is the mass of a...Problem 1.131QP:
Vinegar contains acetic acid (about 5% by mass). Pure acetic acid has a strong vinegar smell but is...Problem 1.132QP:
Ethyl acetate has a characteristic fruity odor and is used as a solvent in paint lacquers and...Problem 1.135QP:
Convert; a 5.91 kg of chrome yellow to milligrams b 753 mg of vitamin A to micrograms c 90.1 MHz...Problem 1.136QP:
Convert: a 7.19 g of cyanocobalamin (vitamin B12) to milligrams b 104 pm, the radius of a sulfur...Problem 1.137QP:
The largest of the Great Lakes is Lake Superior, which has a volume of 12,230 km3. What is this...Problem 1.138QP:
The average flow of the Niagara River is 3.50 km3 per week. What is this volume in liters?Problem 1.141QP:
The masses of diamonds and gems are measured in carats. A carat is defined as 200 mg. If a jeweler...Problem 1.142QP:
One year of world production of gold was 49.6 106 troy ounces. One troy ounce equals 31.10 g. What...Problem 1.144QP:
All good experiments start with a scientific question. What was the scientific question that Art Fry...Problem 1.148QP:
A 33.0-g sample of an unknown liquid at 20.0C is heated to 120C. During this heating, the density of...Problem 1.149QP:
A 124-g sample of a pure liquid, liquid A, with a density of 3.00 g/mL is mixed with a 40.8-mL...Problem 1.150QP:
On a long trip you travel 832 miles in 21 hours. During this trip, you use 31 gallons of gasoline. a...Problem 1.151QP:
The density of lead at 20C is 11.3 g/cm3. Rank the volumes of the following quantities of lead from...Problem 1.154QP:
The density of liquid water at 80C is 972 kg/m3 and at 20C is 998 kg/m3. If you have 200.0 mL of...Problem 1.156QP:
At 20C liquid gasoline gas has a density of 0.75 g/cm3. If a 5.5-mL sample of gasoline is placed...Problem 1.157QP:
The figures below represent a gas trapped in containers. The orange balls represent individual gas...Problem 1.158QP:
An ice cube measures 3.50 cm on each edge and weighs 39.45 g. a Calculate the density of ice. b...Problem 1.159QP:
The total length of all the DNA molecules contained in a human body is 1 1010 miles. The population...Problem 1.160QP:
Prospectors are considering searching for gold on a plot of land that contains 1.31 g of gold per...Problem 1.161QP:
A solution is prepared by dissolving table salt, sodium chloride, in water at room temperature. a...Problem 1.162QP:
Water and saline (salt) solution have in common that they are both homogeneous. How do these...Problem 1.163QP:
When 11.1 g of marble chips (calcium carbonate) is treated with 54.3 mL of hydrochloric acid...Problem 1.164QP:
Zinc ore (zinc sulfide) is treated with sulfuric acid, leaving a solution with some undissolved bits...Problem 1.165QP:
A steel sphere has a radius of 1.58 in. If this steel has a density of 7.88 g/cm3, what is the mass...Problem 1.166QP:
A weather balloon filled with helium has a diameter of 3.50 ft. What is the mass in grams of the...Problem 1.169QP:
A sample of an ethanolwater solution has a volume of 54.2 cm3 and a mass of 49.6 g. What is the...Problem 1.170QP:
You have a piece of gold jewelry weighing 9.35 g. Its volume is 0.654 cm3. Assume that the metal is...Problem 1.171QP:
A sample of vermilion-colored mineral was weighed in air, then weighed again while suspended in...Problem 1.172QP:
A sample of a bright blue mineral was weighed in air, then weighed again while suspended in water....Browse All Chapters of This Textbook
Chapter 1 - Chemistry And MeasurementChapter 1.3 - Law Of Conservation Of MassChapter 1.4 - Matter: Physical State And Chemical CompositionChapter 1.5 - Measurement And Significant FiguresChapter 1.6 - Si UnitsChapter 1.7 - Derived UnitsChapter 1.8 - Units And Dimensional Analysis (factor-label Method)Chapter 2 - Atoms, Molescules, And IonsChapter 2.1 - Atomic Theory Of MatterChapter 2.2 - The Structure Of The Atom
Chapter 2.3 - Nuclear Structure; IsotopesChapter 2.4 - Atomic WeightsChapter 2.5 - Periodic Table Of The ElementsChapter 2.6 - Chemical Formulas; Molecular And Ionic SubstancesChapter 2.8 - Naming Simple CompoundsChapter 2.10 - Balancing Chemical EquationsChapter 3 - Calculations With Chemical Formulas And EquaitonsChapter 3.1 - Molecular Weight And Formula WeightChapter 3.2 - The Mole ConceptChapter 3.3 - Mass Percentages From The FormulaChapter 3.4 - Elemental Analysis: Percentages Of Carbon, Hydrogen And OxygenChapter 3.5 - Determining FormulasChapter 3.6 - Molar Interpretation Of A Chemical EquationChapter 3.7 - Amounts Of Substances In A Chemical ReactionChapter 3.8 - Limiting Reactant; Theoretical And Percentage YieldsChapter 4 - Chemical ReactionsChapter 4.1 - Ionic Theory Of Solutions And Solubility RulesChapter 4.2 - Molecular And Ionic EquationsChapter 4.3 - Precipitation ReactionsChapter 4.4 - Acid-base ReactionsChapter 4.5 - Oxidation-reduction ReactionsChapter 4.6 - Balancing Simple Oxidation-reduction EquationsChapter 4.7 - Molar ConcentrationChapter 4.8 - Diluting SolutionsChapter 4.9 - Gravimetric AnalysisChapter 4.10 - Volumetric AnalysisChapter 5 - The Gaseous StateChapter 5.1 - Gas Pressure And Its MeasurementChapter 5.2 - Empirical Gas LawsChapter 5.3 - The Ideal Gas LawChapter 5.4 - Stoichiometry Problems Involving Gas VolumesChapter 5.5 - Gas Mixtures; Law Of Partial PressuresChapter 5.6 - Kinetic Theory Of An Ideal GasChapter 5.7 - Moleculat Speeds; Diffusion And EffusionChapter 5.8 - Real GasesChapter 6 - ThermochemistyChapter 6.1 - Energy And Its UnitsChapter 6.2 - First Law Of Thermodynamics; Work And HeatChapter 6.3 - Heat Of Reaction; Enthalpy Of ReactionChapter 6.4 - Thermochemical EquaitonsChapter 6.5 - Applying Stoichiometry To Heats Of ReactionChapter 6.6 - Measuring Heats Of ReactionChapter 6.7 - Hess's LawChapter 6.8 - Standard Enthalpies Of FormationChapter 7 - Quantum Theory Of The AtomChapter 7.1 - The Wave Nature Of LightChapter 7.2 - Quantum Effects And PhotonsChapter 7.3 - The Bohr Theory Of The Hydrogen AtomChapter 7.4 - Quantum MechanicsChapter 7.5 - Quantum Numbers And Atomic OrbitalsChapter 8 - Electron Configurations And PeriodicityChapter 8.1 - Electron Spin And The Pauli Exclusion PrincipleChapter 8.2 - Building-up Principle And The Periodic TableChapter 8.3 - Writing Electron Configurations Using The Periodic TableChapter 8.4 - Orbital Diagrams Of Atoms; Hund's RuleChapter 8.6 - Some Periodic PropertiesChapter 8.7 - Periodicity In The Main-group ElementsChapter 9 - Ionic And Covalent BondingChapter 9.1 - Describing Ionic BondsChapter 9.2 - Electron Configurations Of IonsChapter 9.3 - Ionic RadiiChapter 9.5 - Polar Covalent Bonds; ElectronegativityChapter 9.6 - Writing Lewis Electron-dot FormulasChapter 9.7 - Delocalized Bonding: ResonanceChapter 9.8 - Exceptions To The Octet RuleChapter 9.9 - Formal Charge And Lewis FormulasChapter 9.10 - Bond Length And Bond OrderChapter 9.11 - Bond EnthalpyChapter 10 - Molecular Geometry And Chemical Bonding TheoryChapter 10.1 - The Valence-shell Electron-pair Repulsion (vsepr) ModelChapter 10.2 - Dipole Moment And Molecular GeometryChapter 10.3 - Valence Bond TheoryChapter 10.4 - Description Of Multiple BondingChapter 10.6 - Electron Configurations Of Diatomic Moleucles Of The Second-period ElementsChapter 11 - States Of Matter; Liquids And SolidsChapter 11.2 - Phase TransitionsChapter 11.3 - Phase DiagramsChapter 11.5 - Intermolecular Forces; Explaining Liquid PropertiesChapter 11.6 - Classification Of Solids By Type Of Attraction Of UnitsChapter 11.7 - Crystalline Solids; Crystal Lattices And Unit CellsChapter 11.8 - Structures Of Some Crystalline SolidsChapter 11.9 - Calculations Involving Unit-cell DimensionsChapter 12 - SolutionsChapter 12.1 - Types Of SolutionsChapter 12.2 - Solubility And The Solution ProcessChapter 12.3 - Effects Of Temperature And Pressure On SolubilityChapter 12.4 - Ways Of Expressing ConcentrationChapter 12.5 - Vapor Pressure Of A SolutionChapter 12.6 - Boiling-point Elevation And Freezing-point DepressionChapter 12.7 - OsmosisChapter 12.8 - Colligative Properites Of Ionic SolutoinsChapter 12.9 - ColloidsChapter 13 - Rates Of ReactionChapter 13.1 - Definition Of Reaction RateChapter 13.3 - Dependence Of Rate On ConcentrationChapter 13.4 - Change Of Concentration With TimeChapter 13.5 - Temperature And Rate; Collision And Transisiton-state TheoriesChapter 13.6 - Arrhenius EquationChapter 13.7 - Elementary ReactionsChapter 13.8 - The Rate Law And The MechanismChapter 14 - Chemical EquilibirumChapter 14.1 - Chemical Equilbrium - A Dynamic EquilibriumChapter 14.2 - The Equilibrium ConstantChapter 14.3 - Heterogenous Equilibria; Solvents In Homogenous EquilibriaChapter 14.4 - Qualitativelys Interpreting The Equilibrium ConstantChapter 14.5 - Predicting The Direction Of ReactionChapter 14.6 - Calculating Equilibrium ConcentrationsChapter 14.7 - Removing Products Or Adding ReactantsChapter 14.8 - Changing The Pressure And TemperatureChapter 15 - Acids And BasesChapter 15.2 - Bronsted-lowry Concept Of Acids And BassesChapter 15.3 - Lewis Concept Of Acids And BasesChapter 15.4 - Relative Strengths Of Acids And BasesChapter 15.5 - Moleculat Structure And Acid StrengthChapter 15.7 - Solutions Of A Strong Acid Or BaseChapter 15.8 - The Ph Of A SolutionChapter 16 - Acid-base EquilibriaChapter 16.1 - Acid-ionization EquilibriaChapter 16.2 - Polyprotic AcidsChapter 16.3 - Base-ionization Of EquilibriaChapter 16.4 - Acid-base Properties Of Salt SolutionsChapter 16.5 - Common-ion EffectChapter 16.6 - BuffersChapter 16.7 - Acid-base Titration CurvesChapter 17 - Solubility And Complex-ion EquilibriaChapter 17.1 - The Solubility Product ConstantChapter 17.2 - Solubility And The Common-ion EffectChapter 17.3 - Precipitation CalculationsChapter 17.4 - Effect Of Ph On SolubilityChapter 17.5 - Complex-ion FormationChapter 17.6 - Complex Ions And SolubilityChapter 18 - Thermodynamics And EquilibriumChapter 18.2 - Entropy And The Second Law Of ThermodynamicsChapter 18.3 - Strandard Entropies And The Third Law Of ThermodynamicsChapter 18.4 - Free Energy And SpontaneityChapter 18.6 - Relating ?g° To The Equilibrium ConstantChapter 18.7 - Change Of Free Energy With TemperatureChapter 19 - ElectrochemistryChapter 19.1 - Balancing Oxidation-reduction Reactions In Acidic And Basic SolutionsChapter 19.2 - Construction Of Voltaic CellsChapter 19.3 - Notation For Voltaic CellsChapter 19.4 - Cell PotentialChapter 19.5 - Standard Cell Potentials And Standard Electrode PotentialsChapter 19.6 - Equilibrium Constants From Cell PotentialsChapter 19.7 - Dependence Of Cell Potential On ConcentrationChapter 19.8 - Some Commercial Voltaic CellsChapter 19.9 - Electrolysis Of Molten SaltsChapter 19.10 - Aquesous ElectrolysisChapter 19.11 - Stiochiometry Of ElectrolysisChapter 20 - Nuclear ChemistryChapter 20.1 - RadioactivityChapter 20.2 - Nuclear Bombardment ReactionsChapter 20.3 - Radations And Matter: Detection And Biological EffectsChapter 20.4 - Rate Of Radioactive DecayChapter 20.6 - Mass-energy CalculationsChapter 21 - Chemistry Of The Main-group ElementsChapter 21.9 - Group 5a: Nitrogen And The Phosphorus FamilyChapter 21.10 - Group 6a: Oxygen And The Sulfur FamilyChapter 22 - The Transition Elements And Coordination CompoundsChapter 22.3 - Formation And Structure Of ComplexesChapter 22.4 - Naming Coordination CompoundsChapter 22.5 - Structure And Isomerism In Coordination CompoundsChapter 22.7 - Crystal Field TheoryChapter 23 - Organic ChemistryChapter 23.2 - Alkanes And CycloalkanesChapter 23.3 - Alkenes And AlkynesChapter 23.5 - Naming HydrocarbonsChapter 23.6 - Organic Compounds Containing OxygenChapter 24 - Polymer Materials: Synthetic And BiologicalChapter 24.1 - Synthesis Of Organic PolymersChapter 24.3 - ProteinsChapter 24.4 - Nucleic AcidsChapter A.1 - Scientific (exponential) NotationChapter A.2 - LogarithmsChapter A.3 - Algebraic Operations And Graphing
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Chapter 1, Problem 1.1QPChapter 1, Problem 1.57QPChapter 1, Problem 1.58QPChapter 1, Problem 1.65QPChapter 1, Problem 1.66QPChapter 1, Problem 1.67QPChapter 1, Problem 1.68QPChapter 1, Problem 1.69QPChapter 1, Problem 1.70QP
Chapter 1, Problem 1.109QPChapter 1, Problem 1.113QPChapter 1, Problem 1.114QPExplanation: Given mass in problem statement is 8.45 kg . Since, 1 kg = 103 g and 1 μg = 10-6 g , we...Explanation: Given distance in problem statement is 127 Å . Since, 1 Å = 10−10 m and 1 mg = 10-3 g ,...Chapter 1, Problem 1.135QPChapter 1, Problem 1.136QPChapter 1, Problem 1.169QPChapter 1, Problem 1.170QPChapter 2, Problem 2.1QPChapter 2, Problem 2.25QPChapter 2, Problem 2.26QPExplanation: The product in the given chemical equation is Lithium chloride. Hence, the starting...Chapter 2, Problem 2.97QPChapter 2, Problem 2.98QPExplanation: The given reaction in the problem statement is ammonium chloride and barium hydroxide...Explanation: The raw chemical equation given in the problem statement is, C2H6 + O2 → CO2 + H2O The...Chapter 2, Problem 2.126QPExplanation: Molecule is the term that is used for compounds which contain only covalent bonding...Chapter 3, Problem 3.1QPExplanation: To calculate the number of candy pieces in 0.2 kg of candy. Given, 1.0 kg of candy has...Chapter 3, Problem 3.18QPChapter 3, Problem 3.33QPChapter 3, Problem 3.37QPChapter 3, Problem 3.41QPChapter 3, Problem 3.42QPChapter 3, Problem 3.45QPChapter 3, Problem 3.46QPChapter 3, Problem 3.57QPChapter 3, Problem 3.58QPChapter 3, Problem 3.63QPExplanation: To calculate the masses of Carbon, Hydrogen and Oxygen. Molar mass of Carbon is 12.01 g...Explanation: To determine the produced mass of K2SO4 The given reaction is, 2 KOH+ H2SO4→K2SO4 +...Chapter 3, Problem 3.141QPChapter 4, Problem 4.1QPChapter 4, Problem 4.33QPChapter 4, Problem 4.34QPChapter 4, Problem 4.38QPChapter 4, Problem 4.39QPChapter 4, Problem 4.40QPChapter 4, Problem 4.43QPChapter 4, Problem 4.44QPChapter 4, Problem 4.45QPChapter 4, Problem 4.46QPExplanation: The complete molecular equation for the reaction between potassium hydroxide and...Chapter 4, Problem 4.48QPExplanation: The molecular equation for the reaction between HCN and lithium hydroxide is given...Chapter 4, Problem 4.100QPChapter 4, Problem 4.101QPChapter 4, Problem 4.103QPExplanation: Assume that both hydrogen atoms of H2SO4 ionize completely. H2SO4(aq) + Ba(OH)2(aq) →...Explanation: When an object having one kilogram of mass and it is placed in one square meter area...Explanation: Figure 1 According to kinetic theory of gases the molecules in a container are...Explanation: From Ideal gas equation, PV = nRT we can observe that pressure is directly proportional...Explanation: Figure 1 From Ideal gas law, PV = nRT Pressure and volume are inversely proportional to...Chapter 5, Problem 5.32QPExplanation: From the ideal gas equation and density formula, Both the density and pressure are...Explanation: To Calculate: The partial pressure of each of the gases from a certain volcano whose...Explanation: To Calculate: The rms speed (in m/s) of nitrogen (N2) molecules at 25∘C and at 125∘C...Chapter 5, Problem 5.136QPExplanation: Given data: A container is filled with 16.0 g of O2 and 14.0 g of N2 Moles of oxygen:...Chapter 5, Problem 5.147QPChapter 5, Problem 5.153QPExplanation: Given, A sample of Zinc with pressure 751 mmHg and temperature 170C . The level of...Chapter 5, Problem 5.158QPChapter 5, Problem 5.159QPExplanation: Given, An ideal gas with RMS of a gas is 5.00×102m/s and pressure of 2.5 atm and...Explanation: Given, Power plant driven by fossil fuel combustion generate substantial greenhouse...Chapter 6, Problem 6.1QPChapter 6, Problem 6.32QPChapter 6, Problem 6.36QPChapter 6, Problem 6.75QPChapter 6, Problem 6.76QPChapter 6, Problem 6.80QPChapter 6, Problem 6.81QPChapter 6, Problem 6.82QPChapter 6, Problem 6.115QPChapter 6, Problem 6.125QPExplanation: Given information, 2Al(s) + Fe2O3(s) → 2Fe(l) + Al2O3(s)ΔHf : 2 × 0 - 825.5 2 × 12.40...Explanation: Given information, 4KO2(s) + 2H2O(l) → 4KOH(s) + 3O2(g)ΔHof : 4 × - 284.5 2 × -285.8 4...Explanation: Given information, 2Na(s) + 2H2O(l) → 2Na+(aq) + 2OH-(aq) + H2(g)ΔHf : 0 2 × -285.8 2 ×...Explanation: Given information Total mass of hydrogen and oxygen gas is 2.500 g.Temperature is 25 oC...Chapter 6, Problem 6.151QPChapter 6, Problem 6.152QPExplanation: Figure 1 Calculate the HHV for propane by using the trend line equation, Molar mass for...Chapter 7, Problem 7.1QPChapter 7, Problem 7.23QPChapter 7, Problem 7.24QPChapter 7, Problem 7.67QPChapter 7, Problem 7.69QPChapter 7, Problem 7.70QPChapter 7, Problem 7.82QPChapter 7, Problem 7.83QPExplanation: To calculate: The wavelength of emitted light when an electron from hydrogen atom...Chapter 7, Problem 7.105QPChapter 7, Problem 7.106QPChapter 7, Problem 7.108QPChapter 7, Problem 7.112QPChapter 8, Problem 8.1QPExplanation: Bohr formula is ΔE=-RH[22∞2−2212]=-RH[-4]= 4 RH 4 × 2.179×10-18J1 He+ ion I.E= 4 ×...Chapter 9, Problem 9.1QPChapter 9, Problem 9.24QPChapter 9, Problem 9.71QPChapter 9, Problem 9.72QPChapter 9, Problem 9.75QPChapter 9, Problem 9.81QPChapter 9, Problem 9.118QPExplanation: The electronic configuration of Cl atom is Cl17:[Ne]3s2 3p5 But the Chlorine atom gain...Chapter 9, Problem 9.137QPChapter 9, Problem 9.138QPChapter 10, Problem 10.1QPChapter 10, Problem 10.37QPChapter 10, Problem 10.38QPChapter 11, Problem 11.1QPChapter 11, Problem 11.25QPChapter 11, Problem 11.28QPChapter 11, Problem 11.63QPChapter 11, Problem 11.74QPExplanation: Intermolecular force in each compound In a 1-Pentanol, the intermolecular forces are...Explanation: Intermolecular force in each compound CH3CHO is found to be polar molecule, therefore...Chapter 11, Problem 11.157QPExplanation: Gaseous solution is made of gases. One best example for gaseous solution is air – it is...Chapter 12, Problem 12.25QPChapter 12, Problem 12.26QPChapter 12, Problem 12.70QPExplanation: Assume that volume of solution is 1.000 L which is equivalent to 1.040 kg as density of...Explanation: Assume that volume of solution is 1.000 L which is equivalent to 1.127 kg as density of...Chapter 12, Problem 12.95QPChapter 12, Problem 12.96QPChapter 12, Problem 12.107QPChapter 12, Problem 12.108QPExplanation: Parts per million is expressed as, ppm = mass of solutemass of solution × 106 The term...Explanation: Determine the number of moles of each ion present in the solution. Totally five types...Explanation: Determine the number of moles of each ion present in the solution. Totally five types...Chapter 12, Problem 12.141QPChapter 12, Problem 12.142QPChapter 13, Problem 13.1QPChapter 13, Problem 13.27QPExplanation: The reaction follows first order with presence of half-life of ten seconds. There are...Chapter 13, Problem 13.65QPChapter 13, Problem 13.95QPChapter 13, Problem 13.96QPExplanation: Given, Time[CH3NNCH3]0.0min1.50×10-2 M 1.0min1.26×10-2 M2.0min1.10×10-2 M3.0...Explanation: Given, Time[NO2]0.0min0.1103 M 1.0min0.1076 M2.0min0.1050 M3.0 min0.1026 M Time Average...Chapter 13, Problem 13.105QPExplanation: To calculate the concentration of NO2 after 2.5×102 sec The integrated rate law for...Chapter 13, Problem 13.132QPChapter 13, Problem 13.140QPChapter 13, Problem 13.141QPChapter 13, Problem 13.145QPExplanation: The plot of 1[A] (vs) time gives a straight line and the reaction is said to be second...Chapter 13, Problem 13.150QPChapter 14, Problem 14.1QPChapter 14, Problem 14.45QPChapter 14, Problem 14.71QPChapter 14, Problem 14.72QPExplanation: Given, The equilibrium constant Kc =3.92 The initial amount of CO = 1.00 mol The...Explanation: Given, The equilibrium constant Kc =0.153 The initial amount of N2 = 1.00 mol The...Chapter 14, Problem 14.101QPChapter 14, Problem 14.103QPChapter 14, Problem 14.107QPChapter 14, Problem 14.108QPExplanation: Given, Volume of the flask =2.00 L Pressure = 1.00atm Partial pressure of N2=0.781 atm...Explanation: Given, The initial amount of I2 = 0.500 mol The initial amount of Br2 = 0.500 mol The...Chapter 14, Problem 14.137QPChapter 14, Problem 14.138QPChapter 15, Problem 15.1QPChapter 15, Problem 15.20QPChapter 15, Problem 15.35QPChapter 15, Problem 15.36QPChapter 15, Problem 15.53QPChapter 15, Problem 15.54QPChapter 15, Problem 15.85QPChapter 15, Problem 15.99QPChapter 15, Problem 15.100QPExplanation: Illustration of amphiprotic behavior of bicarbonate ion with water by writing...Chapter 15, Problem 15.102QPExplanation: The hydrated aluminum ion acts as Bronsted-Lowry acid and it can react with ammonia a...Chapter 15, Problem 15.119QPExplanation: The equilibrium of the given reaction can be represented as follows. Conc. (M) H3O+(aq)...Chapter 16, Problem 16.1QPChapter 16, Problem 16.21QPChapter 16, Problem 16.22QPChapter 16, Problem 16.47QPChapter 16, Problem 16.91QPChapter 16, Problem 16.92QPChapter 16, Problem 16.113QPChapter 16, Problem 16.114QPChapter 16, Problem 16.116QPChapter 16, Problem 16.119QPChapter 16, Problem 16.120QPChapter 16, Problem 16.129QPChapter 16, Problem 16.130QPChapter 16, Problem 16.135QPExplanation: To Calculate: The pH prior to the addition of any HCl Given data: A 0.150 M solution of...Chapter 16, Problem 16.157QPChapter 17, Problem 17.1QPChapter 17, Problem 17.31QPChapter 17, Problem 17.33QPChapter 17, Problem 17.34QPChapter 17, Problem 17.41QPChapter 17, Problem 17.42QPChapter 17, Problem 17.43QPChapter 17, Problem 17.67QPChapter 17, Problem 17.68QPChapter 17, Problem 17.91QPExplanation: To calculate: The molar solubility of AgI in 2.2 M NH3 . Given, The strength of NH3 is...Explanation: To calculate: The concentration of calcium ion, sodium ion, chloride ion and fluoride...Explanation: To calculate: The quantity of water and ammonia required to dissolve silver chloride....Chapter 17, Problem 17.128QPChapter 18, Problem 18.1QPExplanation: To give: The change in the water sample Given information, temperature of the water is...Explanation: To explain: The change in standard free energy for the given reaction Given reaction...Chapter 18, Problem 18.50QPExplanation: To calculate: the value of ΔHo Given reaction and information ΔHo (kJ)CO2(g) + 2H2(g) →...Chapter 18, Problem 18.88QPExplanation: To calculate: The value of ΔHo and ΔSo for the given reactions For the first reaction,...Chapter 18, Problem 18.92QPChapter 18, Problem 18.97QPChapter 18, Problem 18.98QPExplanation: To calculate: The value of ΔHof The value of standard enthalpy change of formation...Explanation: Given reaction and information 2NH3(g) → 3H2(g) + N2(g)ΔHfo: 2 × -45.90 0 0 kJ So: 2 ×...Explanation: Given reaction and information CO(g) + 3H2(g) → CH4(g) + H2O(g)ΔHfo: -110.5 0 -74.87...Chapter 19, Problem 19.1QPChapter 19, Problem 19.23QPChapter 19, Problem 19.32QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: C2O42- →2CO2 +...Explanation: To write the equations for two half-reactions, Oxidation half reaction: Mn2+ →MnO4- +...Chapter 19, Problem 19.37QPChapter 19, Problem 19.38QPChapter 19, Problem 19.39QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: 8H2S → S8 +...Chapter 19, Problem 19.41QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: H2O2 →O2 + 2e-...Chapter 19, Problem 19.101QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: S2-→ S8...Chapter 19, Problem 19.113QPExplanation: Given: Reduction of 2.0 mol Fe3+ to Fe2+ In above reduction 1 mole of electron is...Explanation: To calculate the cell potential (EMF) of given cell The standard reduction potentials...Explanation: Two types of nuclear reactions are, Radioactive decay Nuclear bombardment reactions...Explanation: Alpha emission ( α ): An unstable nucleus emits 24He nucleus or alpha particle....Explanation: Given nuclear reaction is, 4H11→H24e + 2e10 This reaction is found to be fusion...Explanation: To determine: Nuclear masses of each nucleus Nuclear mass of 12H = 2.01400 amu -...Explanation: To determine: Nuclear mass of 11H nucleus Nuclear mass of 12H = 2.01400 amu -...Explanation: Given: Mass of I-136 nuclei = 135.8401 amu Mass of Y-96 nuclei = 95.8629 amu Nuclear...Explanation: Given: Nuclear mass of 24He= 4.00260 amu-(2×0.000549amu)=4.001502amu Write the...Explanation: When Bromine-82 undergoes beta ( -10β ) decay it gives Krypton-82. This balanced...Explanation: When Tellurium-132 undergoes beta ( -10β ) decay it gives Xenon-132. This balanced...Given incomplete nuclear reaction is, 1431Si→ 1531P + ? This is written as, 1431Si→ 1531P + ZAX...Explanation: To calculate: Mass defect of Sodium Atomic mass of Na = 22.99 amu Mass of eleven...Explanation: Given Mass of electron = 0.000549 amu Temperature = 25°C 2p + 2n→ 24He Nuclear mass of...Explanation: Given Mass of electron = 0.000549 amu Temperature = 25°C 94239Pu→ 92235U + 24H...Explanation: Alloy is a mixture of one or more metals in a solid form. Examples for alloys are...Explanation: Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide...Explanation: To Write: The complete balanced equation for the given incomplete reaction. Potassium...Explanation: To Write: The complete balanced equation for the given incomplete reaction. Lithium...Explanation: To Write: The complete balanced equation for the given incomplete reaction. Barium...Explanation: Given Equation: KOH(aq) + MgCl2(aq)→ Complete Equation: A complete equation will have...Explanation: Given data: Lead(IV) oxide is prepared by oxidizing plumbite ion, Pb(OH)3- which exists...Explanation: Given Equation: Al2O3(s) + H2SO4(aq)→ Complete Equation: A complete equation will have...Explanation: Given Equation: Pb(NO3)2(aq) + Al(s)→ Complete Equation: A complete equation will have...Explanation: Given: The given molecule is ethylene and carbon is group 4A element. Carbon atom has 4...Explanation: Given data: The given cracking reaction is: CH4(g) →C(graphite) + 2H2(g) To Calculate:...Explanation: Given data: The given reaction involving synthesis of gas is: CO(g) + 2H2(g)→ CH3OH(g)...Explanation: Given Equation: CO2(g) + Ba(OH)2(aq)→ Complete Equation: A complete equation will have...Explanation: Given Equation: NaHCO3(aq) + HC2H3O2(aq)→ Complete Equation: A complete equation will...Explanation: Given data: Burning of lithium metal in oxygen. Chemical Equation: The chemical...Explanation: Given data: Burning of calcium metal in oxygen. Chemical Equation: The chemical...Explanation: Given data: Water vapor decomposes to atoms in gas phase. Hydrogen peroxide vapor...Explanation: To write: The complete and balanced equation for given combustion. P4(s) + 5O2(g) →...Explanation: To determine: The percentage of sodium acetate in a mixture of sodium acetate and...Explanation: To write: Chemical equation for given reaction Carbon burns in a air it gives Carbon...Explanation: To write: The reaction between copper and hydrochloric acid, iron and hydrochloric...Chapter 22, Problem 22.1QPExplanation: Atomic number of Vanadium is 23 and its electronic configuration is...Explanation: Atomic number of Zirconium is 40 and its electronic configuration is [Kr]4d25s2 . In...Explanation: In the complex ion [Pt(NH3)2]2+ the central metal ion Platinum is in +2 oxidation state...Explanation: In the complex ion [Pt(NH3)2(NO2)2]2+ the central metal ion Platinum is in +4 oxidation...Explanation: The reaction between Cu2+(aq) , NH3(aq) and [Cu(NH3)4]2+(aq) can be represented as,...Explanation: The reaction between Ag+(aq) , NH3(aq) and [Ag(NH3)2]+(aq) can be represented as,...Explanation: The complex ion [CoF6]3− has six fluoro ligands. Hence, the co-ordination number is six...Explanation: Oxidation state of Chromium in the complex [Cr(H2O)6]3+ , oxidation state of Cr =...Explanation: Oxidation state of Cobalt in the complex [Co(NH3)6]3+ , oxidation state of Co = charge...Chapter 23, Problem 23.1QPExplanation: By looking at the formula of the given compound we can identify that a carbonyl group...Explanation: For First structure: In the given ball-stick model, the black spheres are carbon atoms,...Chapter 23, Problem 23.24QPChapter 23, Problem 23.31QPExplanation: The given reaction in the problem statement is an combustion reaction and hence, the...Explanation: From the given name of the hydrocarbon, the parent carbon is identified as octane....Chapter 23, Problem 23.40QPExplanation: 2-methylpentane has the molecular formula of C6H14 . When this undergoes combustion...Explanation: Differentiation between condensation and addition polymer are as follows, Addition...
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