H₂ stored in a 50.0 L container has a pressure of 500.0 torr. O₂ stored in a 25.0 L container has a pressure of 800.0 torr. If both these gases are released together to be stored in a 100.0 L container, what is the total pressure in the 100.0 L container?

Question

Quizplus · Accepted Answer

The total pressure can be found using the ideal gas law and the principle of partial pressures. First, calculate the moles of each gas using $P_1V_1 = nRT$ (where $R$ and $T$ are constants and can be ignored for this calculation since they are the same for both gases and the process). For the first gas: $n_1 = \frac{P_1V_1}{RT} = \frac{500 \times 50}{RT}$. For the second gas: $n_2 = \frac{P_2V_2}{RT} = \frac{800 \times 25}{RT}$. When combined in a 100.0 L container, the total moles $n_{total} = n_1 + n_2$. The total pressure $P_{total}$ can then be found using $P_{total}V_{total} = n_{total}RT$, where $V_{total} = 100.0 L$. Simplifying, we find $P_{total} = \frac{(500 \times 50 + 800 \times 25)}{100}$ torr = 450 torr.

H2 Stored in a 50

H₂ Stored in a 50