The following sets of values for ${C_V}$ and ${C_P}$ of a gas have been reported by different students. The units are $cal/gm-mole-K$. Which of these sets is most reliable?

If the degree of freedom of a gas is $f,$ then the ratio of two specific heats ${C_P}/{C_V}$ is given by

The figure shows the graph of logarithmic reading of pressure and volume for two ideal gases $A$ and $B$ undergoing an adiabatic process. From the figure, it can be concluded that:

$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

For an ideal non-rigid diatomic gas,the value of $\frac{R}{C_V}$ is nearly,given that $\gamma = \frac{C_P}{C_V} = \frac{9}{7}$.

One mole of an ideal monatomic gas requires $210 \, J$ of heat to raise the temperature by $10 \, K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by $10 \, K$,then the heat required is ....... $J$.