A vessel with a volume of 17.3 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) 117 atm
B) 0 atm
C) 4 atm
D) 3 atm
E) 56 atm

Question

Quizplus · Accepted Answer

To find the total pressure in the vessel, we use the ideal gas law, $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the number of moles of gas, $R$ is the ideal gas constant, and $T$ is the temperature in Kelvin. First, we convert the temperature to Kelvin: $25°C + 273.15 = 298.15 K$. Next, we calculate the moles of each gas: Nitrogen ($N_2$): $2.80 \, \text{g} / 28.02 \, \text{g/mol} = 0.1 \, \text{mol}$ Hydrogen ($H_2$): $0.403 \, \text{g} / 2.02 \, \text{g/mol} = 0.2 \, \text{mol}$ Argon ($Ar$): $79.9 \, \text{g} / 39.95 \, \text{g/mol} = 2 \, \text{mol}$ Total moles of gas = $0.1 + 0.2 + 2 = 2.3 \, \text{mol}$ Using $R = 0.0821 \, \text{L·atm/(K·mol)}$, the pressure can be calculated as: $P = \frac{nRT}{V} = \frac{2.3 \, \text{mol} \times 0.0821 \, \text{L·atm/(K·mol)} \times 298.15 \, \text{K}}{17.3 \, \text{L}} \approx 3 \, \text{atm}$

A Vessel with a Volume of 17