$A$ gaseous mixture contains an equal number of hydrogen $(H_2)$ and nitrogen $(N_2)$ molecules. Specific heat measurements on this mixture at temperatures below $100\, K$ would indicate that the value of $\gamma$ (ratio of specific heats) for this mixture is

Two rigid boxes placed on a table contain different ideal gases. Box $A$ contains $1 \text{ mole}$ of nitrogen at temperature $T_0$. Box $B$ contains $1 \text{ mole}$ of helium at temperature $(7/3) T_0$. Both boxes are brought into thermal contact,and heat flows until they reach a common final temperature $T_f$. (Neglect the heat capacity of the boxes). Express the final temperature $T_f$ in terms of $T_0$.

$A$ mixture of hydrogen and oxygen has volume $500 \, cm^3$,temperature $300 \, K$,pressure $400 \, kPa$,and mass $0.76 \, g$. The ratio of the mass of oxygen to the mass of hydrogen is:

When one mole of monatomic gas is mixed with one mole of a diatomic gas,then the equivalent value of $\gamma$ for the mixture will be (vibration mode neglected).

Two gases have the same pressure $P$,temperature $T$,and volume $V$. If they are mixed and the final volume and temperature remain $V$ and $T$ respectively,what will be the final pressure?

If three moles of monoatomic gas $\left(\gamma=\frac{5}{3}\right)$ is mixed with two moles of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$,the value of adiabatic exponent $\gamma$ for the mixture is: