The ratio of two specific heats $\frac{C_P}{C_V}$ of $CO$ is

The molar specific heat at constant pressure of an ideal gas is $(7/2)R$. The ratio of specific heat at constant pressure to that at constant volume is

If $C_{p}$ and $C_{v}$ are molar specific heats of an ideal gas at constant pressure and volume respectively and $\gamma$ is $C_{p} / C_{v}$,then $C_{p} =$ (where $R$ is the universal gas constant).

$1 \, mole$ of a gas requires $40 \, calories$ of heat to raise its temperature from $20^{\circ}C$ to $30^{\circ}C$ at constant pressure. How many calories of heat are required to raise the temperature of the same gas by the same amount at constant volume? $(R = 2 \, cal \, mol^{-1} K^{-1})$

Explain the difference between the expressions $C_P - C_V = R$,$C_P - C_V = \frac{R}{J}$,and $C_P - C_V = \frac{r}{J}$.

$176 \text{ grams}$ of $CO_2$ can change its temperature from $0^{\circ} C$ to $30^{\circ} C$ by absorbing $3600 \text{ joules}$ of thermal energy. The molar specific heat of $CO_2$ in $J \ mol^{-1} K^{-1}$ is: