Unit Ten: Gases
Review Packet
Name: _______________________
Hour: _____
1.
As your elevation increases, what happens to the pressure and why?
2.
Why do snow shoes allow you to walk on the top of snow without sinking?
3.
What is standard pressure for the following units
a. __________ atm
b.
__________ kPa
c.
__________ mm Hg
d.
__________ psi
4.
637 mm Hg is equivalent to how many atm?
5.
What is the ideal gas law?
6.
As pressure increases and the number of moles and volume are held constant, the temperature will
_________________.
7.
As volume increases and the number of moles and pressure are held constant, the temperature will
_________________.
8.
As volume increases and the pressure and temperature remain constant, the number of moles will
_________________.
9.
As volume increases and the number of moles and temperature remain constant, the pressure will
_________________.
10. When using the gas laws, what unit MUST temperature be in?
11. Convert the temperatures below.
a.
37°C = __________ K
f.
267 K
= __________ °C
b.
0.0°C = __________ K
g.
342 K
= __________ °C
c.
-52°C = __________ K
h.
108 K
= __________ °C
d.
91°C
= __________ K
i.
298 K
= __________ °C
e.
-112°C = __________ K
j.
317 K
= __________ °C
12. When welding, a common gas mixture is 82.0% argon and 18.0% carbon dioxide. If the total pressure is
736 mmHg, what are the partial pressures of argon and carbon dioxide?
13. What is the temperature in °C of 2.31 moles of a gas that occupies 9.32 L at 4.65 atm?
14. If a balloon occupies 1.09 L at room temperature (25.0°C), what temperature would you need to increase
the volume to 2.98L?
15. If you transfer a gas at room temperature (25.0°C ) from a 9.89 L cylinder to a 2.01 L container and the
pressure increases from 0.623 atm to 1.76 atm, what is the final temperature?
16. If there is a pressure of 633 mmHg in a container and it is heated from 25.0°C to 100.0°C, what is the new
pressure?
17. If you blow up a balloon with helium gas and the volume increases from 5.60 mL to 1006 mL and there are
initially 0.103 moles, how many moles need to be added?
18. A hand pump with a moveable piston has an applied pressure of 4.08 atm and a volume of 3.49L. What is
the volume if the applied pressure is decreased to 1.27 atm?
19. 4.58 grams of dry ice (CO2) sublime to occupy a 5.00 L container at 25.0°C. What is the pressure?
20. Calculate the new pressure when 8.31 L of a gas at 649 mmHg is compressed to 7.09 L.
21. A gas mixture contains helium, oxygen, and an unknown gas. Calculate the partial pressure (in atm) of the
unknown gas when the partial pressure of helium is 523 mmHg, oxygen is 168 mmHg, and the total
pressure is 1.13 atm.
22. If the temperature of 0.508 L of gas is increased from 72.0°C to 115.0°C, what is the new volume?
23. If the pressure changes from 2.19 atm at room temperature (25.0°C) to 0.825 atm, what is the final
temperature?
24. If you increase the number of moles of a gas from 0.213 moles to 0.879 moles and the initial volume is
78.0 mL, what is the final volume?
25. How many liters will 89.5 grams of Br2 occupy at a pressure of 749 mmHg and a temperature of 95.0°C?
26. A sample of gas has a temperature of 4.4°C, a volume of 251 mL and a pressure of 649 mmHg. What will
happen to the volume if the temperature increases to 25.0°C and the pressure becomes 761 mmHg?
27. If 34.8 L of Cl2 react with an unlimited supply of H2 at STP, how many moles of HCl would be produced?
H2 (g) + Cl2 (g) → 2 HCl (g)
28. If 5.29 moles of NO react with an unlimited supply of oxygen gas at 654 mmHg and 78.0°C, what volume
of NO2 will be produced?
2 NO (g) + O2 (g) → 2 NO2 (g)
29. How much faster does NH3 diffuse than HCl?
30. If helium effuses 4.80 times faster than an unknown gas sample, what is the molar mass of the unknown
gas?