A mixture of two moles of hydrogen and one mo | vedclass

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(B) According to the kinetic theory of gases,the average kinetic energy of a gas molecule depends only on the absolute temperature $T$ and is given by

Vedclass · Accepted Answer

Statement $(i)$ is correct while statement $(ii)$ is incorrect.

Vedclass · Answer

(B) According to the kinetic theory of gases,the average kinetic energy of a gas molecule depends only on the absolute temperature $T$ and is given by $K_{av} = \frac{3}{2} kT$. Since both gases are at the same room temperature,the average kinetic energy per molecule is the same for both $H_2$ and $Ar$. Thus,statement $(i)$ is correct.For an ideal gas mixture in a closed container,the partial pressure $p_i$ of a component is given by $p_i = \frac{n_i}{n_{total}} P_{total}$. Since the number of moles of hydrogen $(n_{H_2} = 2)$ is greater than the number of moles of argon $(n_{Ar} = 1)$,the partial pressure of hydrogen will be greater than the partial pressure of argon. Thus,statement $(ii)$ is incorrect.

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