In a gas mixture, the total pressure is the sum of partial pressures; equal volumes of gases do not possess equal masses; diffusion rate is proportional to molecular mass.
The total pressure of the mixture of gases is the sum of the partial pressures. In a gas mixture, each individual gas exerts a pressure known as its partial pressure, and the total pressure of a gas mixture is the sum of these partial pressures according to Dalton's Law of Partial Pressures.
At the same temperature and pressure, equal volumes of gases possess equal masses. This statement is incorrect as equal volumes of gases do not necessarily possess equal masses since different gases have different molar masses.
The rate of diffusion of gases is directly proportional to their molecular mass. This statement is true as the rate of diffusion of gases is inversely proportional to the square root of their molar masses according to Graham's Law of Effusion.
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