Gas Law CW 1
R = 8.314
L ikPa
mol iK
and
R = 0.0821
L iatm
mol iK
Ideal Gas Law Problems
1. At what temperature will 1.05 mol of argon gas exert a pressure of 115 kPa
in a 5.21 L container?
2. What volume does 2.15 mol of nitrogen gas occupy at 273 K and 1.02 atm?
3. What is the pressure in atm, in a 245 L tank that contains 5.21 kg of helium,
mm = 4.0026 g/mol, at 27°C?
4. What mass of helium gas is needed to pressurize a 100.0 L tank to 255 atm at
25°C?
5. What mass of oxygen gas, mm = 32.998 g/mol, would be required to fill a
tank similar to that in problem number 4?
6. At what temperature will a 1.0 g sample of neon gas, mm = 20.180 g/mol,
exert a pressure of 345 kPa in a 5.0 L container?
7. Determine the pressure of a 20 L tank containing 0.845 mol of oxygen gas
and 0.495 mol of hydrogen gas at 23°C.
Derived Gas Law Problems
8. Calculate the final pressure of a 20.0 L tank of chlorine gas initially at 1.00
atm that is compressed down to 18.0 L.
9. A 0.55 L balloon at 0°C is heated to 23°C. Calculate its new volume.
10. A 15.0 L tank of argon gas initially at STP is compressed to 13.5 L and heated
to room temperature (23°C), determine the new pressure.
11. Calculate the final pressure of a tank of chlorine gas initially at STP
containing 3.5 moles of gas when an additional 1.5 moles of gas is added.
Gas Law CW 1 Solutions
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Ideal Gas Law Problems
At what temperature will 1.05 mol of argon gas exert a pressure of 115 kPa
in a 5.21 L container?
(115) (5.21) = 1.05 (8.314) T
T = 68.6K
What volume does 2.15 mol of nitrogen gas occupy at 273 K and 1.02 atm?
1.02 V = 2.15 (0.0821) (273)
V = 47.2 L
What is the pressure in atm, in a 245 L tank that contains 5.21 kg of helium,
mm = 4.0026 g/mol, at 27°C?
5210 / 4.0026 = 1302 mol He
P (245) = (1302) (0.0821) (300)
P = 131 atm
What mass of helium gas is needed to pressurize a 100.0 L tank to 255 atm at
25°C?
255 (100.0) = n (0.0821) (298)
n = 1042 moles (4.0026) = 4200 g or 4.20 kg
What mass of oxygen gas, mm = 32.998 g/mol, would be required to fill a
tank similar to that in problem number 4?
1042 (32.998) = 34.4 kg
At what temperature will a 1.0 g sample of neon gas, mm = 20.180 g/mol,
exert a pressure of 345 kPa in a 5.0 L container? 1 / 20.180 = 0.0496 mol
345 (5.0) = (0.0496) (8.314) T
T = 4200 K
Determine the pressure of a 20 L tank containing 0.845 mol of oxygen gas
and 0.495 mol of hydrogen gas at 23°C.
P (20) = 1.34 (0.0821) (296)
P (20) = 1.34 (8.314) (296)
P = 1.63 atm
165 kPa
Derived Gas Law Problems
8. Calculate the final pressure of a 20.0 L tank of chlorine gas initially at 1.00
atm that is compressed down to 18.0 L.
P1V1 = P2V2
(1.00) (20.0) = P2 (18.0)
P2 = 1.11 atm
9. A 0.55 L balloon at 0°C is heated to 23°C. Calculate its new volume.
V1 / T1 = V2 / T2
0.55 / 273 = V2 / 298
V2 = 0.60 L
10. A 15.0 L tank of argon gas initially at STP is compressed to 13.5 L and heated
to room temperature (23°C), determine the new pressure.
P1V1 / T1 = P2V2 / T2
(1.00)(15.0) / 273 = P2(13.5) / 298
P2 = 1.21 atm
11. Calculate the final pressure of a tank of chlorine gas initially at STP
containing 3.5 moles of gas when an additional 1.5 moles of gas is added.
P1 / n1 = P 2 / n2
1.00 / 3.5 = P2 / 5.0
P2 = 1.4 atm