$A$ container holds $8 \, g$ of $O_2$ and $7 \, g$ of $N_2$ at a pressure of $10 \, atm$. If $O_2$ is removed,the pressure becomes ... $atm$.

In a container,there is a mixture of two different gases. Will both gases have the same kinetic energy?

One mole of a gas having $\gamma = \frac{7}{5}$ is mixed with one mole of a gas having $\gamma = \frac{4}{3}$. The value of $\gamma$ for the mixture is ($\gamma$ is the ratio of the specific heats of the gas).

$1 \text{ mole}$ of ideal monoatomic gas $(\gamma_1 = 5/3)$ is mixed with $1 \text{ mole}$ of diatomic gas $(\gamma_2 = 7/5)$. What is $\gamma$ for the mixture? $\gamma$ denotes the ratio of specific heat at constant pressure to that at constant volume.

$1 \, g$ of $H_2$ at $27 \, ^oC$ is mixed with $16 \, g$ of $O_2$ at $37 \, ^oC$. The temperature of the mixture is about ....... $^oC$.

$2\, moles$ of helium gas is mixed with $3\, moles$ of hydrogen molecules (taken to be rigid). What is the molar specific heat of the mixture at constant volume in $J/mol\, K$? $(R = 8.3\, J/mol\, K)$