A vessel with a volume of 10.1 L contains 3.28 g of nitrogen gas, 0.400 g of hydrogen gas, and 85.0 g of argon gas. At 26.0°C, what is the pressure in the vessel?

Question

Quizplus · Accepted Answer

1. Calculate the moles of each gas using the ideal gas law: PV = nRT.

- For nitrogen gas: n(N2) = (3.28 g)/(28.0134 g/mol) = 0.117 mol
- For hydrogen gas: n(H2) = (0.400 g)/(2.01588 g/mol) = 0.199 mol
- For argon gas: n(Ar) = (85.0 g)/(39.948 g/mol) = 2.13 mol

2. Calculate the total moles of gas:

n(total) = n(N2) + n(H2) + n(Ar) = 2.46 mol

3. Calculate the total pressure using the total number of moles and the total volume:

P(total) = (n(total)RT)/V = [(2.46 mol)(0.08206 L*atm/mol*K)(299.15 K)]/(10.1 L) = 5.94 atm

Therefore, the answer is D) 5.94 atm.

A Vessel with a Volume of 10