A gas-mixture consists of two gases, A and B, each with equal mass. Molar mass of B is greater than that of A. which one of the two gases will contribute more to the total pressure of the gas mixture?

Explanation

In a gas mixture, the component gas with higher partial pressure will have greater contribution to the total pressure of the mixture. Masses of A and B in the mixture are the same but the molar mass of B is greater than that of A. hence, in the mixture, the number of moles or the mole fraction `(x_(A))` of A will be greater than that `(x_(B))` of B. suppose, in the mixture, the partial pressures of A and B are `p_(A) and p_(B)` respectively and the total pressure P. according to Dalton's law of partial pressurs, `p_(A)=x_(A)P and p_(B)=x_(B)P`
As, `x_(A) gt x_(B),p_(A)` will be greater than `p_(B)`.
hence, the contribution of gas A to the total pressure of the mixture will be more than that of gas B.