Lab 2 Report 2

Solve question 26 and 27

Part 1. A lightly inflated balloon is placed in a freezer. Explain the change to the size of the balloon based on the kinetic molecular theory.Part 2. What would most likely happen to the balloon if it was instead kept outside in the sun for some time? Explain your answer based on the kinetic molecular theory.In both cases, assume the balloon is tied tight enough so that air does not escape.

Part 1. A glass bottle, which is half-filled with water, has a balloon attached to its opening. The bottle is placed in a hot water bath for some time. Explain the change to the size of the balloon based on the kinetic molecular theory.Part 2. What would most likely happen to the balloon if the bottle was then placed into a jar of cold water with ice cubes? Explain your answer based on the kinetic molecular theory.In both cases, assume the balloon is attached tightly enough so that air does not escape the system.

Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn mineral requires 10 mL of commercial HCl of 37% purity, by weight and density 1.19 g/mL, to react completely. Find: a) The mass of zinc contained in the sample. b) The purity of the zinc mineral. c) The pressure exerted by the hydrogen gas collected in a 2 L container and at a temperature of 20ºC.please use conversion factors and mark the solutionsThe solutions should be : 3,92 g; 78,4%; 0,72 atm.I just dont know how to do it

Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn mineral requires 10 mL of commercial HCl of 37% purity, by weight and density 1.19 g/mL, to react completely. Find: a) The mass of zinc contained in the sample. b) The purity of the zinc mineral. c) The pressure exerted by the hydrogen gas collected in a 2 L container and at a temperature of 20ºC.please use conversion factors and mark the solutions

The world burns approximately 3.7 * 1012 kg of fossil fuel per year. Use the combustion of octane as the representative reaction and determine the mass of carbon dioxide (the most significant greenhouse gas) formed per year. The current concentration of carbon dioxide in the atmosphere is approximately 399 ppm (by volume). By what percentage does the concentration increase each year due to fossil fuel combustion? Approximate the average properties of the entire atmosphere by assuming that the atmosphere extends from sea level to 15 km and that it has an average pressure of 381 torr and average temperature of 275 K. Assume Earth is a perfect sphere with a radius of 6371 km.

Choices: I only II only III only I and II II and III I and III I, II, III None of the above   5. SURFACE TENSION: I. A decrease is due to the weakening of the hydrogen bonds of water molecules II. It is increased when a surfactant is added III. Soap lowers surface tension of water resulting to the shrinkage of molecules on the surface 6. SAPONIFICATION: I. Can be carried out with HCl II. NaOH undergoes hydrolysis III. Its principle is used to determine the number of milligrams of KOH required to neutralize the fatty acids from the complete hydrolysis of 1g of fat 7. HYDROGENATION: I. Involves hydrogen addition across carbon-carbon double bonds II. The removal of a double bond results to an increase in melting point III. Favors the absorption of vitamins in the structure 8. RANCIDITY: I. Oxygen acts as an oxidizing agent at carbon to carbon double bonds II. The products are glycerol and carboxylic acids III. Can be carried out by a certain…

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A student constructs a simple constant volume gas thermometer and calibrates it using the boiling point of water, 100°C, and the freezing point of a specific brine solution, -17°C. The pressures measured at the calibration points are 1.366 atm and 0.9267 atm, respectively.   **when explaining please use math symbols & equations rather than typing it out, gets confusing if something is in a fraction or whatnot. Thank you!

1. There are 135 L of gas in a container at a temperature of 260°C. If the gas was cooled until the volume decreased to 75 L, what would the temperature of the gas be? 2. CaCO3 decomposes at 1200 degrees Celsius to form CO2 gas and CaO. If 25 L of CO2 are collected at 1200 degrees Celsius, what will the volume of this gas be after it cools to 25 degrees Celsius? 3. A 2.50 L volume of hydrogen measured at -196 degrees Celsius is warmed to 100 degrees Celsius. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.

7. According to the researchers, the burning of 11.5 grams of alcohol yielded 22.0 grams of carbon dioxide and 13.5 grams of water in an experiment. Find out what the empirical formula of the chemical is by using the following formula: 8.  Research for five comprehensive examples of problems on gas laws.  You should provide an answer key (along with a solution or solutions).

1. What is the mass of a water molecule in grams? 2. A chemist analyzed a sample of a compound that was known to contain potassium, manganese, and oxygen. She obtained the following results: The total mass of the sample = 316.08 g Mass of potassium = 78.20 g Mass of manganese = 109.88 g Determine the percentage composition of the compound 3. If at S.T.P 4.48 L of NH3(g) is allowed to react with 9.03 x 1022 molecules of O₂(g), please answer the questions for the following reaction: 4NH3(g) + 5O₂(g) 6H₂O(g) + 4NO(g) a. What is the limiting reactant? Please show all your work. b. What mass of nitrogen monoxide can be expected? c. If 3.00 g of nitrogen monoxide recovered, what would the percentage yield be? d. What reactant is in excess? Following the reaction, what is the remaining mass of the excess reactant?

1. Hot air balloonists turn a propane flame on and off to control their balloon. What effect does the propane burner have when the flame is on? Explain why hot air rises, using the kinetic molecular theory of gases.  2. When the air in a hot-air balloon is heated, what physical property of air changes that causes the hot air balloon to rise? Use the kinetic molecular theory of gases in your explanation.

A student is given a 72 g sample of liquid water. This liquid sample was boiled until it was completely water vapor (gas) . what will be the volume of the sample if all the water vapor is kept @ STP ?

In the lab, 42.0 mL of hydrogen gas is collected over water. The water temperature is recorded to be 25.2 C. The pressure of the collected gas is measured to be 762.0 mm Hg. What is the partial pressure of the hydrogen gas that was collected? Note: The vapor pressure of water at 25.2 C is 24.0 mm Hg.

By placing a bottle of hydrochloric acid next to another of ammonia and removing the corks from both, we note the formation of intense white smoke, consisting of ammonium chloride (HCl + NH3→ NH4Cl).  This experience is an example of:   a. decomposition     b. combination     c. sublimation     d. double replacement     e. single replacement

1. A cylinder containing 15.0 L of helium gas at a pressure of 165 atm is to be used to fill party balloons. Each balloon must be filled to a volume of 2.0 L at a pressure of 1.1 atm. What is the maximum number of balloons that can be inflated? Assume that the gas in the cylinder is at the same temperature as the inflated balloons. (HINT: The “empty” cylinder will still contain helium at 1.1 atm.). 2. For a gas sample whose total pressure is 740 torr, what are the partial pressures if the moles of gas present are 1.3 mol of N2, 0.33 mol of O2, and 0.061 mol of Ar?

Please answer question 72 please. Thank you!

when you open a can of soda that has just been shaken, the contents will spray out. This spraying is an illustration of which gas law? 1. Boyles Law 2. Avogards Law 3. Charles Law

1.  Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant? 2.  Why does the density of water change with its temperature? 3.  If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation? 4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?

Read the description below of a substance and an experiment on it. Decide whether the result of the experiment tells you the substance is a pure substance or a mixture, if you can. • The sample is a solid yellow cube with a total mass of 50.0 g. The cube is put into a pressure chamber and the pressure raised by pumping in nitrogen gas. At a pressure of 55. atm an orange liquid is observed seeping from the cube. After 30 minutes this flow stops, and the smaller and lighter-colored cube sits in a puddle of orange liquid without further change. Is the sample made from a pure substance or a mixture? If the description of the substance and the outcome of the experiment isn't enough to decide, choose "can't decide." pure substance Omixture (can't decide) X S ? A olo Ar 1

1. Carbon dioxide gas has an initial pressure of 650 mmHg and an initial volume of 0.50 L. At constant temperature and in a closed-system, what is the pressure (in atm) when the volume of the sample is decreased to 125 mL? 2. Under constant pressure, a sample of hydrogen gas initially at 88.0 °C and 9.40 L is cooled until its final volume is 2.50 L. What is its final temperature in the unit of Kelvin? 3. Given that 35.5 g of carbon monoxide are present in a container if volume 250 mL. What is the pressure of the gas (in atm) if the temperature is 55 °C. 4. What volume is occupied by 15.5 g of argon gas at a pressure of 820 mmHg and a temperature of 50.0 °C? Would the volume be different if the sample were 15.5 g of chlorine gas (under identical conditions)?