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Gas Laws Worksheet #1 - Boyle’s, Charles’, Gay-Lussac’s, and Combined Gas Law

Solve all problems – you must show your work (including units). The correct answer is given in parentheses at the end of the problem.

Boyle’s Law

1. A gas sample contained in a cylinder equipped with a moveable piston occupied 300.0 mL at a pressure of 2.00 atm. What would be the final pressure if the volume were increased to 500.0 mL at constant temperature? (1.20atm)

2. A balloon that contains 1.50 L of air at 1.00 atm is taken underwater to a depth at which the pressure is 3.00 atm. Calculate the new volume of the balloon. Assume that the temperature remains constant. (0.500L)

3. A 50.0 L sample of gas collected in the upper atmosphere at a pressure of 18.3 torr is compressed into a 150.0 mL container at the same temperature. A. What is the new pressure, in atm? B. To what volume would the original sample have had to be compressed to exert a pressure of 10.0 atm? (A. 8.03atm; B. 0.120L)

Charles’ Law

1. Several balloons are inflated with helium to a volume of 0.75 L at 27(C. One of the balloons was found several hours later, the temperature had dropped to 22(C. What would be the volume of the balloon when found, if no helium has escaped? (0.74L)

2. A weather balloon is filled to the volume of 150.0 L on a day when the temperature is 10.0(C. If no gases escaped, what would be the volume of the weather balloon after it rises to an altitude where the temperature is -8.00(C? (140.L)

3. A fixed quantity of gas at 23.0(C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is increased to 145(C while the pressure is held constant. (14.5L)

4. A sample of gas occupies a volume of 7.50 L at 0.988 atm and 28.0(C. At what temperature, in degrees Celsius, is the volume of the gas 4.00 L if the pressure is kept constant. (-112(C)

Gay-Lussac’s Law

1. A sample of gas occupies 10.0 L at 100.0 torr and 27.0(C. Calculate the pressure if the temperature is changed to 127(C while the volume remains constant. (133 torr)

2. The temperature of 200.0 mL of a gas originally at STP changes to -25(C at constant volume. Calculate the pressure of the gas in atm. (0.91atm)

3. A gas occupies a volume of 50.0 mL at 27(C and 630 mmHg. At what temperature, in (C, would the pressure be 101.3 kPa if the volume remains constant? (89(C)

4. A sample of gas occupies a volume of 5.00 L at 700. mmHg and 30.0(C. At what temperature, in (C, would the pressure be 600. torr if the volume remains constant? (-13.3(C)

Moles and Volume Law

1. A 5.50 mole sample of gas has a volume of 2.50L. What would be the volume if the amount increased to 11.0 moles? (5.00 L)

2. 7.50 moles of nitrogen occupies 4.25 L. How many moles of nitrogen would be present if the volume were 12.5 L, assuming pressure and temperature remain constant? (22.1 mol)

3. 2.15 moles of oxygen occupies 650. mL. How many moles of oxygen would be present if the volume were 1300. mL, assuming pressure and temperature remain constant? (4.30 mol)

Combined Gas Law

1. A 280.0 mL sample of neon exerts a pressure of 660.0 torr at 26.0(C. At what temperature, (C, would it exert a pressure of 940. torr in a volume of 440.0 mL if the number of moles remains constant? (396(C)

2. A certain gas has a volume of 500.0 mL at 77.0(C and 600.0 torr. Calculate the temperature, (C, if the volume decreased to 400.0 mL and the pressure increases to 1.00 atm and the number of moles remains constant. (81.9(C)

3. A given sample of gas has a volume of 4.20 L at 60.0(C and 1.00 atm pressure. Calculate its pressure if the volume is changed to 5.00 L and the temperature to 27(C (assume the amount of gas does not change). (0.76atm)

4. 4.50 moles of a certain gas occupies a volume of 550.0 mL at 5.000(C and 1.000 atm. What would the volume be if 10.50 moles were present at 27.00(C and 1.250 atm? (1107 mL)

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Gas Law Worksheet #2 (Dalton’s Law, Ideal Gas Law, and Graham’s Law)

Solve all problems – you must show your work (including units). The correct answer is given in parentheses at the end of the problem.

Dalton’s Law

1. Determine the total pressure of a gas mixture that contains oxygen at a pressure of 150.mmHg, nitrogen at 350.mmHg pressure, and helium at a pressure of 200.mmHg. Give you answer in mmHg and in atm. (700.mmHg, 0.921atm)

2. A gas mixture containing oxygen, nitrogen, and carbon dioxide has a pressure of 250.mmHg. If the partial pressure of oxygen is 50.0mmHg and the partial pressure of nitrogen is 175mmHg, what is the partial pressure of the carbon dioxide? (25.0mmHg)

3. The volume of oxygen collected over water is 18.5 mL at 25.0(C and 600.torr. Calculate the dry volume of the oxygen if the temperature and pressure changed to STP. Hint: First determine the partial pressure of the oxygen and then use the Combined Gas Law to determine the new volume. (12.9mL)

4. Consider a mixture of two gases A and B, confined to a closed vessel. A quantity of a third gas, C, is added to the same vessel at the same temperature. How does the addition of gas C affect the following:

A. the partial pressure of gas A, B. the total pressure in the vessel?

5. If a gas is collected over water at 30.0(C into a 100.mL container and the pressure is 645 torr, what would be the pressure of just the gas at 5.00(C in the same container? Hint: First determine the partial pressure of the gas and then use Gay-Lussac’s Law to determine the new pressure. (562torr)

Ideal Gas Law

1. A chemist is preparing to carry out a reaction at high pressure that requires 36.0 moles of hydrogen gas. The chemist pumps the hydrogen into a 12.4 L rigid steel container at 25.0 (C. To what pressure, in atm, must the hydrogen be compressed? (71.0atm)

2. To what temperature, in (C, must 10.0 grams of NH3 gas have to be heated in a 15.0 L container in order for it to exert a pressure of 3.50 atm? (816(C )

3. 2.00X10-3 grams of hydrogen gas at 155 (C exert a pressure of 323 torr on the walls of a small cylindrical tube. What is the volume of the tube? (0.0819L)

4. It is desired to obtain a volume of 1000.mL of nitrogen at 100.(C and 640.torr. How many grams of nitrogen would be required? (0.771g)

5. Some oxygen is collected in a 250.mL container at 25.0(C and 720.mmHg. How many moles of oxygen is this? (0.00968mol)

6. What is the pressure, in torr, of a gas occupying 1.07L at 12.0(C and containing 0.0448 moles of gas? (745 torr)

8. What is the molar mass of a gas if 475mL of it has a mass of 0.0740 grams. The temperature at the time of the measurement was 100.(C and the pressure is 1.0663 X 105 Pa. (4.54 g/mol)

Graham’s Law

1. Place the following gases in order of increasing average molecular speed at 300. K: CO2, N2O4, F2, HF, and H2. Think about the mass of each gas!!!

2. What is the relative rate of diffusion between hydrogen and nitrogen? (H2 diffused 3.72 times faster.)

3. What is the relative rate of diffusion between oxygen and carbon dioxide? (O2 diffused 1.17 times faster.)

4. At a certain temperature the velocity of chlorine molecules is 0.0410 m/s. What is the velocity of sulfur dioxide at the same temperature and pressure? (0.0431 m/s)

6. A certain gas effuses four times as fast as oxygen. What is the molar mass of this gas? (2.00 g/mol)

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Gas Worksheet #3 – Molar Volume and Gas Stoichiometry

Solve problems using dimensional analysis. You may have to write a balanced chemical equation for some of the problems. Show all work, answers are given at the end of the problem.

Molar Volume

1. Calculate the number of moles contained in 550.mL of carbon dioxide at STP. (0.0246mol)

2. Calculate the mass of 1.50 L of CH4 at STP. (1.07g)

3. Calculate the volume in liters of 50.0 grams of nitrogen dioxide at STP. (24.3L)

Gas Stoichiometry

1. Given the following reaction: NH4NO2 (s)( N2 (g) + 2H2O (g) How many liters of nitrogen gas is produced if 50.0L of water is produced at STP? (25.0L)

2. Given the following reaction: CuO (s) + H2 (g) ( Cu (s) + H2O (g) If 250. L of hydrogen gas are used to reduce copper (II) oxide at STP, what mass of copper is to be expected? (709g)

3. How many grams of solid lithium must be added to liquid water in order to obtain 15.0 L of hydrogen gas at STP? (9.29g)

4. When black gunpowder explodes, solid potassium nitrate, solid carbon, and solid sulfur react with each other to form nitrogen gas, carbon dioxide gas, and solid potassium sulfide. If the original mixture contains 50.0 grams of potassium nitrate, what volume of carbon dioxide is produced in the reaction at STP? (16.6L)

5. Calculate the volume of hydrogen gas at produced by the reaction of 0.52 grams of solid magnesium with excess hydrochloric acid. (0.48L)

6. How many liters of hydrogen gas are needed to react completely with 50.0 L of chlorine gas at STP? How many liters of hydrogen chloride gas is produced in the reaction? (a.50.0L; b.100.L)

7. Given the following reaction: 2NO (g) + O2 (g) ( 2NO2 (g) How many liters of gaseous oxygen are needed to produce 4.50 L of gaseous nitrogen dioxide, if both gases are being measured at STP? (2.25L)

8. Given the following reaction: N2 (g) + 3H2 (g)( 2NH3 (g) If 200. L of ammonia are produced in the reaction between nitrogen and hydrogen at STP, how many liters of nitrogen and hydrogen gases are used up in this reaction? (100. L nitrogen, 300. L hydrogen)

9. Given the following reaction: F2 (g) + H2 (g)( 2HF (g) If 30.0 L of fluorine gas are exposed to 50.0 L of hydrogen gas at STP which is the limiting reactant? Which is the excess? How many liters of hydrogen fluoride are formed in this reaction? (fluorine is limiting, hydrogen is excess, 60.0L)

10. If 1800.L of C2H2 are burned in oxygen, how many liters of carbon dioxide gas are formed? (3600.L)

Solids, Liquids, and Gases Test Review

Read over the notes and practice problems.

1. Be able to define and identify the 6 phase changes (freezing, melting, vaporization, condensation, sublimation, and deposition).

2. Gases have a definite volume. True or False? 3. Solids have a definite volume. True or False?

4. Liquids have a definite volume. True or False? 5. Gases have a definite shape. True or False?

6. Solids have a definite shape. True or False? 7. Liquids have a definite shape. True or False?

8. Solids are considered fluids. True or False? 9. Liquids are considered fluids. True or False?

10. Gases are considered fluids. True or False?

11. Draw a picture showing the structure of a solid, liquid, and gas:

12. Define compressibility: (use drawing from above if needed)

13. Define the following terms: intermolecular forces and intramolecular forces

14. List the 3 intermolecular forces: 15. List the 3 intramolecular forces:

16. Be able to define and identify the 6 phase changes (freezing, melting, vaporization, condensation, sublimation, and deposition).

17. Solids and liquids have _____________________forces while gases have little to none. This is why gases do not have a definite volume or shape.

18. Dipole-dipole, London dispersion, and hydrogen bonding are intermolecular forces. True or false?

19. Intermolecular forces describe the forces of attraction between one molecule and another molecule. True or false?

20. Intramolecular forces describe the bonds between atoms within a molecule. True or false?

21. Gases have little to no intermolecular forces so they have no definite shape or volume. True or false?

22. Covalent, ionic, and metallic bonding are the three intramolecular forces. True or False?

23. Ionic bonds are the strongest of the three intramolecular forces. True or False?

24. Which phase changes involve the forming of intermolecular forces?

25. Which phase changes involve the breaking of intermolecular forces?

Solve the following problems. For some problems you may have to write a balanced chemical equation. The answers are given in ( ) at the end of each problem

1. A gas is heated from –20.0( C to 57.0( C and the volume is increased from 2.00 L to 4.50 l. If the initial pressure is 0.125 atm, what is the final pressure? (0.0725 atm)

2. The volume of a sample of gas is 650.mL at 0.00(C. What volume will the sample occupy at 75.0(C? (829.ml)

3. 7.50 moles of nitrogen occupies 4.25 L. How many moles of nitrogen would be present if the volume were 12.5 L, assuming pressure and temperature remain constant? (22.1 mol)

4. A 4.40 grams piece of solid carbon dioxide is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 300. K. What is the pressure of the gas? (2.46 atm)

5. The mass of 1.12 liters of gas Y is found to be 6.23 grams. What is the molar mass of Gas Y at STP? (125 g/mol)

6. It is found that 250.mL of gas at STP has a mass of l.00 gram. What is the molar mass of this gas? (89.6 g/mol)

7. In the reaction 2KClO3 (s)( 2KCl (s) + 3O2 (g), oxygen gas is collected over water at 25.0(C in a 4.00 L tank at a total pressure of 884 mmHg. What is the pressure of the dry oxygen? How many moles of oxygen were produced in this reaction? (860.mmHg; 0.185moles)

8. What happens to the pressure of a gas if the temperature in Kelvin is tripled and the volume is decreased by a factor of 9?

9. A gas is collected over water at 35.0( C into a 500.ml flask and the pressure is found to be 0.993atm. What would be the pressure of the dry gas at 95.0(C if the volume did not change? (1.12atm)

10. Gas X is found to effuse four times faster than argon. What is the molar mass of the unknown gas? (2.50g/mol)

12. A certain gas effuses five times as fast as krypton. What is the molar mass of this gas? (3.35g/mol)

13. If 120.grams of copper (II) oxide are decomposed, what volume of oxygen is produced (at STP)? (16.9L)

14. When 70.0 grams of hydrogen peroxide, H2O2, are decomposed to water and oxygen gas, how many liters of oxygen are released (at STP)? (23.0L)

15. How many grams of potassium chlorate are required in the preparation of 90.0 liters of oxygen (at STP)? (328g)

16. In the electrolysis of 144 grams of water, how many liters of hydrogen are produced (at STP)? (179L)

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