Question

Suppose you have a mixture of ideal gases. Which of the following statements is false? Select one: a. The mixture will behave as an ideal gas to a first approximation. b. The molar volume depends on the identity of the gases c. The gases will expand to fill the entire container. The total pressure is equal to the sum of partial pressures of the constituent d. gases.

Answer 1

a.) Since all are ideal gases and do not interact with each other, it can be assumed that the mixture will also behave as an ideal gas. Therefore the statement is correct.

b.) Since the gases have neither any attractive nor any repulsive forces acting upon them, the constituent gases will have their partial molar volumes intact and the total molar volume of the mixture will be equal to the sum of those partial molar volumes of the constituent gases. Hence, this statement is FALSE.

c.) The gases have no forces but only collisions, through which they can occupy any volume of the container, i.e. the statement is correct.

d.) According to Dalton's Law (i.e.The total pressure of a mixture of gases is the sum of the partial pressures of the individual constituent gases), this statement is also correct.