When heat $Q$ is supplied to a diatomic gas of rigid molecules at constant volume,its temperature increases by $\Delta T$. The heat required to produce the same change in temperature at constant pressure is:

An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is

The quantity of heat required to raise the temperature of one mole of a monoatomic gas by one degree Kelvin at constant volume is

Using the law of equipartition of energy, the specific heat (in $J\, kg^{-1}\, K^{-1}$) of aluminium at room temperature can be estimated to be (atomic weight of aluminium $= 27$).

$105 \, cal$ of heat is required to raise the temperature of $3 \, moles$ of an ideal gas at constant pressure from $30^{\circ} C$ to $35^{\circ} C$. The amount of heat required in calories to raise the temperature of the gas through the range ($60^{\circ} C$ to $65^{\circ} C$) at constant volume is ........ $cal$ $(\gamma = \frac{C_p}{C_v} = 1.4)$.

When heat is supplied to a diatomic gas,it expands at constant pressure. What fraction of the heat supplied is converted into internal energy?