An ideal mono-atomic gas is taken through a process such that $dQ = 3dU$. The molar heat capacity for this process is: (in $R$)

If $\Delta Q$ is the amount of heat supplied to $n$ moles of a diatomic gas at constant pressure,$\Delta U$ is the change in internal energy,and $\Delta W$ is the work done,then the ratio $\Delta W : \Delta U : \Delta Q$ is

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

When an ideal diatomic gas is heated at constant pressure,the fraction of the heat utilized to increase the internal energy of the gas is

$A$ triatomic,diatomic,and monatomic gas are supplied the same amount of heat at constant pressure. Then:

What is the significance of the heat capacity ratio $\gamma = \frac{C_{P}}{C_{V}}$ for a gas?