A vessel with a volume of 10.2 L contains 3.12 g of nitrogen gas, 0.590 g of hydrogen gas, and 82.4 g of argon gas. At 25.4°C, what is the pressure in the vessel?

Question

Quizplus · Accepted Answer

1. Calculate the number of moles of each gas using PV=nRT:
n(N2) = (3.12 g)/(28.01 g/mol) = 0.111 mol
n(H2) = (0.590 g)/(2.02 g/mol) = 0.292 mol
n(Ar) = (82.4 g)/(39.95 g/mol) = 2.06 mol
2. Calculate the total number of moles:
n(total) = n(N2) + n(H2) + n(Ar) = 2.46 mol
3. Calculate the total pressure using PV=nRT:
P = (nRT)/V = [(2.46 mol)(0.0821 L·atm/mol·K)(25.4+273 K)]/10.2 L = 5.92 atm 
Therefore, the answer is D, which is 5.92 atm.

A Vessel with a Volume of 10