A vessel with a volume of 12.4 L contains 2.80 g of nitrogen gas,0.403 g of hydrogen gas,and 79.9 g of argon gas.At 25°C,what is the pressure in the vessel?
A)164 atm
B)256.2 atm
C)4.54 atm
D)0.380 atm
E)2.27 atm

Question

Quizplus · Accepted Answer

1. Calculate the moles of each gas:
n(N2) = 2.80 g / 28.0134 g/mol = 0.0999 mol
n(H2) = 0.403 g / 2.01588 g/mol = 0.2001 mol
n(Ar) = 79.9 g / 39.948 g/mol = 2.001 mol

2. Calculate the total moles of gas:
n(total) = 0.0999 mol + 0.2001 mol + 2.001 mol = 2.301 mol

3. Use the ideal gas law to calculate the pressure:
PV = nRT
P = nRT/V
P = (2.301 mol)(0.08206 L·atm/mol·K)(298 K) / 12.4 L
P = 4.54 atm

Therefore, the pressure in the vessel is 4.54 atm.

A Vessel with a Volume of 12