Question

A mixture of 0.50 mol H2(g) and 0.50 mol N2(g) is introduced into a 15.0 liter container having a pinhole leak at 30oC. After a period of time, which of the following is true?

Answer 1

Answer:

316liter container

Explanation:

thanks you

Answer 2

The true statement is : (b) The partial pressure of N2 exceeds that of H2 in the container.

• The question is based on Graham's Law of effusion that compares the rate of effusion of two gases under similar conditions.
• According to the law, the rate of effusion of a gas is inversely proportional to its molar mass if the temperature and pressure are constant.
• Since the mass of N₂ (14g) > H₂ (2g), hence the rate of effusion is more for hydrogen than nitrogen.
• This means, that more hydrogen escapes out of the container in a given time than nitrogen.
• So, after a period of time, the partial pressure of N₂ exceeds that of H₂ in the container.

(The complete question is: A mixture of 0.50 mol H2(g) and 0.50 mol N2(g) is introduced into a 15.0 liter container having a pinhole leak at 30oC. After a period of time, which of the following is true?

(a) The partial pressure of H2 exceeds that of N2 in the container.

(b) The partial pressure of N2 exceeds that of H2 in the container.

(c) The partial pressures of the two gases remain equal.

(d) The partial pressures of both gases increase above their initial values. )