Mixed Gas Law Worksheet
Answers available at end
Name: ________________
(show your work)
period: _____
Convert:
100 mmHg = _________ kPa
300 mmHg = _________ atm
120 atm
= _________ mmHg
300 torr = _________ kPa
25 kPa
= _________ mmHg
25 mmHg = _________ atm
300oC = _____ K
150K = _____oC
5000oC = _____K
300K = _____ oC
-255oC = _____ K
3500K = _____oC
200oC = _____oF
95oF = _____oC = _____K
45oF = _____oC = _____K
1) A 70. liter sample of gas initially at 280oC is allowed to cool at constant pressure, what
will the new volume be at 0oC?
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
2) A 4.0 liter sample of gas initially at 25oC is allowed to cool at constant pressure, what
will the new volume be at -5oC?
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
3) A buoyancy vest (used in scuba diving) is filled to a volume of 2.3 liters at a pressure of 1
atmosphere (at the surface where the temperature is a balmy 300K), what will the
volume of air be in the vest when the diver dives to a depth of about 90 feet where the
temperature is 17oC and the pressure is 4 atmospheres?
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
4) A 35 liter sample of gas is initially at 15oC and 800 mmHg. Conditions are changed to
303K and 1.5 atm, what is the new volume of the gas?
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
5) Which gas would diffuse faster from the surface of a planet water vapor (H2O) or oxygen (O2)?
How many times faster?
(H = 1, O = 16) (can you understand why most people think that
Mars is “dry”)
6) How many liters of Chlorine gas could be collected at 800 mmHg and 35oC if you decompose
60.0 grams of silver(I) chloride according to the following equation?
(Ag = 107.8, Cl = 35.5)
(Write and balance the equation; Do the stoichiometery at S.T.P first then convert to the given
conditions or use the ideal gas equation)
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
7. In a certain experiment a sample of helium in a vacuum system was compressed at 25 °C
from a volume of 200.0 mL to a volume of 0.240 mL where its pressure was found to be
30.0 mm Hg. What was the original pressure of the helium?
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
8. A hydrogen gas volume thermometer has a volume of 100.0 cm3 when immersed in an
ice-water bath at 0 °C. When immersed in boiling liquid chlorine, the volume of the
hydrogen at the same pressure is 87.2 cm3. Find the temperature of the boiling point of
chlorine in °C.
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
9. 2.50 grams of XeF4 is introduced into an evacuated 3.00 liter container at 80.0 °C. Find
the pressure in atmospheres in the container. (convert to moles at S.T.P first then convert to
the given conditions or use the ideal gas equation)
P1 =
P2 =
V1 =
V2 =
T1 =
T2 =
10. A lighter-than-air balloon is designed to rise to a height of 6 miles at which point it will
be fully inflated. At that altitude the atmospheric pressure is 210 mm Hg and the
temperature is -40 °C. If the full volume of the balloon is 100,000.0 L, how many
kilograms of helium will be needed to inflate the balloon? (determine the volume at S.T.P;
convert to moles; convert to grams then kilograms or use the ideal gas equation)
11. How many liters of pure oxygen, measured at 740 mm Hg and 24 °C, would be required
to burn 1.00 g of benzene, C6H6 (l), to carbon dioxide and water? (Hint: find the moles of
oxygen needed from the balanced equation, then use gas laws.)
12. Air from the prairies of North Dakota in winter contains essentially only nitrogen,
oxygen, and argon. A sample of air collected at Bismarck at -22 °C and 98.90 kPa had
78.0 % N2, 21.0% O2, and 1.0% Ar. Find the partial pressures of each of these gases.
13. For a mole of ideal gas, sketch a graphs of
a. P vs. V at constant T.
b. P vs. T at constant V.
c. V vs. T at constant P.
14. What would be the partial pressure of N2 in a container at 50 °C in which there is 0.20
mole N2 and 0.10 mole CO2 at a total pressure of 101.3 kPa?
15. What volume of Ne at one atm and 25.0 °C would have to be added to a sign having a
volume of 250 mL to create a pressure of one mm Hg at that temperature?
16. Find the volume: gas at 800.0 mmHg and 40.0 °C if its volume at 720.0 mmHg and 15.0
°C is 6.84 L.
17. 12.8 L of a certain gas are prepared at 100.0 kPa and -108 °C. The gas is then forced into
an 855 mL cylinder in which it warms to room temperature, 22.0 °C. Find the pressure of
this gas in kilopascals.
18. In a laboratory experiment, 85.3 mL of a gas are collected at 24 °C and 733 mm Hg
pressure. Find the volume at STP.
19. What is the mass of 18.9 L of NH3 at 31.0 °C and 97.97 kPa?
20. 0.279 moles of O2 in a 1.85 L cylinder exert a pressure of 3.68 atm. What is the
temperature in the cylinder (in °C)?
21. A quantity of potassium chlorate is selected to yield, through heating, 75.0 mL of O2
when measured at STP. If the actual temperature is 28 °C and the actual pressure is 0.894
atm, what volume of oxygen will result?
22. A mixture of hydrocarbons contains three moles of methane, four moles of ethane, and
five moles of propane. The container has a volume of 124 liters and the temperature is 22
°C. Find the partial pressures of the three gases, in kPa.
23. How many liters of H2 at 23 °C and 733 mm Hg are released by the reaction between
1.98 grams of Na and unlimited water by the following equation?
2 Na + 2 H2O -- > H2 + 2 NaOH
Answers: Mixed Gas Law Worksheet
Convert:
100 mmHg = ___13.3___ kPa
300 mmHg = ___0.395_ atm
120 atm
300 torr = _40.0___ kPa
= _91 200___ mmHg
25 kPa
= __188____ mmHg
25 mmHg = __0.033__ atm
300oC = _573__ K
150K = __-123_oC
5000oC = __5 273___K
300K = _27__ oC
-255oC = _18__ K
3500K = __3227___oC
200oC = __392_oF
_280.2__K
95oF = _35__oC = __308_K
45oF = __7.2___oC =
Answers: 1) 34.6 mL 2) 3.6 L 3) 0.56L 4) 25.84 L 5) H2O is 1.33 times faster 6)
5.03 L
7) 0.0360 mm Hg 8) -35 °C 9) 0.117 atm 10) 5.8 kg 11) 2.35 L 12) 77.1 kPa N2, 20.8 kPa
O2, .989 kPa Ar
13) a - hyperbola, b&c - straight lines 14) 67.5 kPa N2, 34 kPa CO2 15) 0.329 mL 16) 6.69 L
17) 2680 kPa
18) 75.6 mL 19) 12.5 g 20) 24.6 °C 21) 92.5 mL 22) 59.3 kPa methane, 79.0 kPa ethane,
98.8 kPa propane
23) 1.08 L