The molar specific heat of an ideal gas at constant pressure and constant volume is $C_p$ and $C_v$ respectively. If $R$ is the universal gas constant and the ratio of $C_p$ to $C_v$ is $\gamma$,then $C_v=$

The relation between two specific heats of a gas is

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 $c_p$ and $c_v$ denote the specific heats (per unit mass) of an ideal gas of molecular weight $M$,then which of the following relations holds true,where $R$ is the molar gas constant?

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?

The correct relation between $\gamma = \frac{C_p}{C_v}$ and temperature $T$ is: