Question

In a container of volume 16.62 m$^3$ at 0°C temperature, 2 moles of oxygen, 5 moles of nitrogen and 3 moles of hydrogen are present, then the pressure in the container is (Universal gas constant = 8.31 J/mol K)

• A. 1570 Pa
• B. 1270 Pa
• C. 1365 Pa
• D. 2270 Pa

Hint:

Ideal gas law: $PV=nRT$. Temperature in Kelvin: $T(K) = T(^\circ C) + 273$.

Answer 1

The Correct Option is C

We can use the ideal gas law: $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the total number of moles, $R$ is the universal gas constant, and $T$ is the temperature in Kelvin. $V = 16.62$ m$^3$ $T = 0^\circ C = 273$ K $n = 2 + 5 + 3 = 10$ moles $R = 8.31$ J/mol K $P = \frac{nRT}{V} = \frac{(10)(8.31)(273)}{16.62} = \frac{22698.3}{16.62} \approx 1365.5$ Pa.