Question

A and B are ideal gases. At T(K), 2 L of A with a pressure of 1 bar is mixed with 4 L of B with a pressure of P\(_B\) bar in a 100 L flask. The pressure exerted by gaseous mixture is 0.1 bar. What is the value of P\(_B\) in bar?

• A. 0.04
• B. 0.02
• C. 0.10
• D. 0.05

Hint:

Use the ideal gas law and Dalton's Law to calculate the partial pressures of each gas in a mixture. The total pressure is the sum of the partial pressures.

Answer 1

The Correct Option is B

We can apply Dalton's Law of partial pressures. The total pressure exerted by the mixture is the sum of the partial pressures of each gas: \[ P_{\text{total}} = P_A + P_B \] Using the ideal gas law, \( P = \frac{nRT}{V} \), we can calculate the partial pressures. For gas A: \[ P_A = \frac{n_A RT}{V_A} = \frac{1 \times RT}{2}
\text{(since \( P_A \) is given)} \] For gas B, the partial pressure is calculated similarly, and we find that the value of \( P_B = 0.02 \) bar.