1. What do you call the pressure exerted by individual gas in mixture?

A. minimum B. maximum C. partial D. total

2. When all of the individual pressures of gases in a mixture was combined, how is it called then?

A. minimum B. maximum C. partial D. total

3. In a mixture of gases in a container, what collision gives rise to the pressure?

A. Collisions between molecules B. Collisions of molecules to the walls

C. Collisions of molecules outside the container D. Collisions of molecules inside and outside the container

4. Pressure of a gas depends on different factors, which of the following does NOT affect pressure of a gas?

A. No. of moles B. no. of bonds C. temperature D. volume

For items 5-7, refer to the problem: A mixture of nitrogen, oxygen and neon gases exerts a total pressure of 493 torr. If the mole fractions of these three

gases are 0.53, 0.14, 0.33 respectively, what will be the individual pressures of these gases?

5. What is the partial pressure of nitrogen?

A. 69.02 torr B. 162.69 torr C. 261.29 torr D. 493 torr

6. What will be the value if you calculated the partial pressure of oxygen?

A. 69.02 torr B. 162.69 torr C. 261.29 torr D. 493 torr

7. What is the partial pressure exerted by the neon gas?

A. 69.02 torr B. 162.69 torr C. 261.29 torr D. 493 torr

8. If 90.0 L of nitrogen is collected over water at 40.0 °C when the atmospheric pressure is 1000.0 mm Hg, what is the partial pressure of the nitrogen?

Water vapor partial pressure at 40.0 °C is 7.4 kPa. Convert if necessary.

A. 55. 52 mm Hg B. 504 mm Hg C. 704 mm Hg D. 1704 mm Hg

9. 20.0 liters of oxygen is collected over water at 50.0 °C. The atmospheric pressure in the room is 105.00 kPa. What is the partial pressure of the

oxygen? 50 °C = 12. 3 kPa

A. 92.7 kPa B. 93.7 kPa C. 94.7 kPa D. 95.7 kPa

10. There is a mixture of 3 moles of hydrogen gas, 7 moles of oxygen, 10 moles of helium, and 5 moles of nitrogen in a closed container. What is the total

number of moles in this system?

A. 10 B. 15 C. 20 D. 25

For item 11-12, refer to this problem: If there is a mixture of hydrogen and oxygen gas in a container with 13 moles total and the mole ratio of hydrogen is 0.67

molHydrogen to 1 moltotal, how many moles of each gas are there?

11. How many moles of hydrogen is present in the mixture?

A. 8.71 B. 10.71 C. 12.71 D. 14.71

12. What is the number of moles of oxygen?

A. 4.09 B. 4.19 C. 4.29 D. 4.39

For items 13-16, use this problem: 24.0 L of nitrogen gas at 2 atm and 12.0 L of oxygen gas at 2 atm are added to a 10 L container at 273 K. Find the partial

pressure of nitrogen and oxygen and then find the total pressure.

13. Using the formula PV=nRT, what will be the number of moles of oxygen?

A. 0.356 B. 0.536 C. 0.653 D. 0. 656

14. What is the total pressure of the mixture in terms of atm?

A. 3.60 B. 3.61 C. 3.62 D. 3.63

15. By rearranging the formula for Dalton’s law, what is the partial pressure of oxygen?

A. 1.20 atm B. 1.21 atm C. 1.22 atm D. 1.23 atm

16. What is the calculated partial pressure of nitrogen?

A. 2.40 atm B. 2.41 atm C. 2.42 atm D. 2.43 atm

For items 17-20, refer to this problem: In a laboratory experiment, 98 g of oxygen and 140 g nitrogen are combined in a 5.0 L at 298 K. Calculate for partial

pressure of each gas and its total pressure.

17. How many moles of oxygen are in the mixture?

A. 1.5 mol B. 2.5 mol C. 3.5 mol D. 4.5 mol

18. In the problem above, what is the partial pressure of oxygen gas?

A. 17.09 atm B. 17.10 atm C. 17.11 atm D. 17.12 atm

19. According to the problem, what is partial pressure exerted by a 140 g nitrogen?

A. 24.45 atm B. 24.50 atm C. 24.55 atm D. 24.60 atm

20. From the given situation, what will be the total pressure of the mixture?

A. 41.47 atm B. 41.57 atm C. 41.67 atm D. 41.77 atm​