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:

$A$ cylinder with fixed capacity of $67.2 \, L$ contains helium gas at $STP$. The amount of heat needed to raise the temperature of the gas by $20 \, ^oC$ is ..... $J$ [Given that $R = 8.31 \, J \, mol^{-1} \, K^{-1}$]

Which one of the following is $NOT$ a correct expression for an ideal gas?
[$C_{P}=$ Molar specific heat of a gas at constant pressure,
$C_{V}=$ Molar specific heat of a gas at constant volume,
$\gamma=$ Ratio of two specific heats of a gas,$R=$ Universal gas constant]

The average degree of freedom per molecule of a gas is $6$. The gas performs $25 \ J$ work,while expanding at constant pressure. The heat absorbed by the gas is .... $J$

Given below are observations on molar specific heats at room temperature of some common gases.

Gas	Molar specific heat $(C_v)$ $(cal\, mol^{-1}\, K^{-1})$
Hydrogen	$4.87$
Nitrogen	$4.97$
Oxygen	$5.02$
Nitric oxide	$4.99$
Carbon monoxide	$5.01$
Chlorine	$6.17$

The measured molar specific heats of these gases are markedly different from those for monatomic gases. Typically,molar specific heat of a monatomic gas is $2.92 \; cal/mol\; K$. Explain this difference. What can you infer from the somewhat larger (than the rest) value for chlorine?

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