Question

A 2.14-L container of H2(g) at 764 mm Hg and 24∘C is connected to a 3.09-L container of He(g) at 729 mm Hg and 24∘C. After mixing, what is the total gas pressure, in millimeters of mercury, with the temperature remaining at 24 ∘C?

Answer 1

To find the total gas pressure after mixing the two gases, we can use Dalton's law of partial pressures. According to Dalton's law, the total pressure exerted by a mixture of non-reacting gases is the sum of the partial pressures of each gas.

Given: Container 1 (H2): Volume (V1) = 2.14 L Pressure (P1) = 764 mm Hg

Container 2 (He): Volume (V2) = 3.09 L Pressure (P2) = 729 mm Hg

We need to find the total pressure (P_total) after mixing.

To use Dalton's law, we assume that the gases behave ideally (no interactions or reactions between the gases) and that the temperature remains constant.

Since the temperature remains at 24 °C, which is 297 K, we can directly use the pressures provided in mm Hg.

Applying Dalton's law, the total pressure is given by: P_total = P1 + P2

Substituting the given values: P_total = 764 mm Hg + 729 mm Hg P_total = 1493 mm Hg

Therefore, the total gas pressure, after mixing the two gases at 24 °C, is 1493 mm Hg.