One mole of a gas mixture is heated under constant pressure,and the heat supplied $Q$ is plotted against the temperature difference $\Delta T$ acquired. Find the approximate value of $\gamma$ for the mixture.

Three moles of oxygen are mixed with $2 \, moles$ of helium. What will be the ratio of specific heats at constant pressure and constant volume for the mixture?

The temperature of the mixture of one mole of helium and one mole of hydrogen is increased from $0^{\circ}C$ to $100^{\circ}C$ at constant pressure. The amount of heat delivered will be ...... $cal$.

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

In a cubic container of inner side length $10 \ cm$, nitrogen gas at $100 \ kPa$ pressure is maintained at $300 \ K$. If the pressure inside the container is increased to $300 \ kPa$ by adding oxygen gas, the ratio of the number of $N_2$ molecules to $O_2$ molecules in the container is:

$14 \, g$ of $CO$ at $27^{\circ} C$ is mixed with $16 \, g$ of $O_2$ at $47^{\circ} C$. The temperature of the mixture is .......... $^{\circ} C$ (vibration mode neglected).