$176 \text{ grams}$ 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:

$A$ gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume $(C_v)$ to the specific heat of gas at constant pressure $(C_p)$ will be.

The specific heat of helium at constant volume is $12.6 \ J \ mol^{-1} \ K^{-1}$. The specific heat of helium at constant pressure in $J \ mol^{-1} \ K^{-1}$ is about (Assume the temperature of the gas is moderate,universal gas constant,$R=8.314 \ J \ mol^{-1} \ K^{-1}$)

To an ideal triatomic gas $800 \,cal$ heat energy is given at constant pressure. If vibrational mode is neglected,then energy used by gas in work done against surroundings is ......... $cal$.

The specific heat at constant pressure $(C_P)$ is greater than the specific heat at constant volume $(C_V)$ for the same gas because:

For all gases,$C_P - C_V$ is a constant. Does this imply that for all gases,$\frac{C_P}{C_V}$ is also a constant?