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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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Mehreen Nisar Mehreen Nisar
wrote...
4 years ago
There is hydrogen gas in a 5.00 L container and nitrogen gas in a 8.00 L container. Both containers are at STP. What will be the total pressure in the 8.00 L container, if all of the hydrogen gas is pumped into the container with the nitrogen gas?
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wrote...
#1
4 years ago
Let's get the moles of the two gases.

Recall: One mole of an ideal gas will occupy a volume of 22.4 liters at STP:   (1 mol=22.4 L)

Hydrogen: 5.00 L * 1 mol/22.4 L = 0.2232
Nitrogen: 8.00 L * 1 mol/22.4 L = 0.3571

Recall:
PV = nRT
R = 0.0821 atm•L/mol•K
T = 273.15 @ STP

P = ntotalRT/V
P = (0.2232 + 0.3571)(0.0821)(273.15)/(8+5)
P = 1.00 atm
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