Chapter 05 – Gases
Chapter 05
Gases
1.
What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure
is 736 mmHg and h = 9.2 cm?
2.
What will happen to the height (h) of the column of mercury in the manometer shown below if the stopcock is opened?
Chapter 05 – Gases
3.
What will happen to the height (h) of the mercury column in the manometer shown below if the stopcock is opened, given
that the atmospheric pressure is 755 mmHg?
Chapter 05 – Gases
4. A pressure that will support a column of Hg to a height of 256 mm would support a column
of water to what height? The density of mercury is 13.6 g/cm3; the density of water is 1.00
g/cm3.
5. The pressure of a gas sample was measured to be 654 mmHg. What is the pressure in kPa?
(1 atm = 1.01325 105 Pa)
Chapter 05 – Gases
6. A sample of pure oxygen gas has a pressure of 795 torr. What is the pressure of the oxygen
in units of atmospheres?
7. Which of these properties is/are characteristic(s) of gases?
Chapter 05 – Gases
8. A sample of pure nitrogen has a temperature of 15C. What is the temperature of the
nitrogen in units of Kelvin?
9. Which of the following describes Dalton’s Law?
Chapter 05 – Gases
10. Which of the following statements is consistent with Boyle’s Law concerning an ideal
gas?
11. At constant temperature, the volume of the container that a sample of nitrogen gas is in is
doubled. As a result the pressure of the nitrogen gas is halved. The amount of nitrogen gas is
unchanged in this process. This is an example of:
Chapter 05 – Gases
12. At constant temperature and volume, a sample of oxygen gas is added to a sample of
nitrogen gas. The pressure of the mixture is found by adding the pressures of the two
individual gases. This is an example of:
13. A sample of a gas occupies 1.40 103 mL at 25C and 760 mmHg. What volume will it
occupy at the same temperature and 380 mmHg?
Chapter 05 – Gases
14. A sample of oxygen gas has a volume of 545 mL at 35C. The gas is heated to 151ºC at
constant pressure in a container that can contract or expand. What is the final volume of the
oxygen gas?
15. A 45 mL sample of nitrogen gas is cooled from 135ºC to 15C in a container that can
contract or expand at constant pressure. What is the new volume of the nitrogen gas?
Chapter 05 – Gases
16. A sample of helium gas occupies 355mL at 23C. If the container the He is in is expanded
to 1.50 L at constant pressure, what is the final temperature for the He at this new volume?
17. The gas pressure in an aerosol can is 1.8 atm at 25C. If the gas is an ideal gas, what
pressure would develop in the can if it were heated to 475C?
Chapter 05 – Gases
18. If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by
what factor does the volume of the sample change?
19. If the pressure of a gas sample is tripled and the absolute temperature is quadrupled, by
what factor will the volume of the sample change?
Chapter 05 – Gases
20. A small bubble rises from the bottom of a lake, where the temperature and pressure are
4C and 3.0 atm, to the water’s surface, where the temperature is 25C and the pressure is 0.95
atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.
21. The temperature of a sample of argon gas in a 365 mL container at 740. mmHg and 25C
is lowered to 12C. Assuming the volume of the container and the amount of gas is
unchanged, calculate the new pressure of the argon.
Chapter 05 – Gases
22. 0.820 mole of hydrogen gas has a volume of 2.00 L at a certain temperature and pressure.
What is the volume of 0.125 mol of this gas at the same temperature and pressure?
23. At what temperature will a sample of nitrogen gas with a volume of 328 mL at 15C and
748 mmHg occupy a volume of 0.898 L at a pressure of 642 mm Hg? Assume the amount of
the nitrogen gas does not change.
Chapter 05 – Gases
24. At what temperature will a sample of oxygen gas with a volume of 0.110 L at 12C and
822 mmHg occupy a volume of 345 mL at a pressure of 578 mm Hg? Assume the amount of
the oxygen gas does not change.
25. Calculate the number of moles of gas contained in a 10.0 L tank at 22C and 105 atm. (R
= 0.08206 Latm/Kmol)
Chapter 05 – Gases
26. Calculate the volume occupied by 35.2 g of methane gas (CH4) at 25C and 1.0 atm. R =
0.08206 Latm/Kmol.
27. Calculate the volume occupied by 56.5 g of argon gas at STP.
Chapter 05 – Gases
28. Calculate the grams of SO2 gas present at STP in a 5.9 L container.
29. Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25C. R = 0.08206
Latm/Kmol.
Chapter 05 – Gases
30. A gas evolved during the fermentation of sugar was collected. After purification its
volume was found to be 25.0 L at 22.5C and 702 mmHg. How many moles of gas were
collected?
31. How many atoms of He gas are present in a 450 mL container at 35C and 740 mmHg?
Chapter 05 – Gases
32. How many atoms of Ar gas are present in a 340 mL container at 55C and 720 mmHg?
33. Calculate the mass, in grams, of 2.74 L of CO gas measured at 33C and 945 mmHg.
34. A 250 mL flask contains 3.4 g of neon gas at 45C. Calculate the pressure of the neon gas
inside the flask.
Chapter 05 – Gases
35. Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will
be exerted by 2,500 g of oxygen gas (O2) when stored at 22C in a 40.0 L cylinder?
36. Calculate the density, in g/L, of N2 gas at 35C and 0.98 atm pressure.
Chapter 05 – Gases
37. Calculate the density of CO2(g) at 120C and 790 mmHg pressure.
38. Calculate the density of Br2(g) at 59.0C and 1.00 atm pressure.