$N$ moles of an ideal diatomic gas is enclosed in a cylinder at temperature $T$. suppose on supplying heat to the gas, its temperature remains constant but $n$ moles get dissociated into atoms. Heat supplied to the gas is

Since the gas is enclosed in a vessel, therefore, during heating process, volume of the gas remains constant. Hence, no work is done by the gas. It means heat supplied to the gas is used to increase its internal energy only.

Initial internal energy of the gas is ${\text{U}}_1=\text{N}\left(\frac{5}{2}\text{R}\right)\text{T}$

Since n moles get dissociated into atoms, therefore, after heating, vessel contains $\left(\text{N}-\text{n}\right)$  moles of diatomic gas and 2n moles of a mono-atomic gas. Hence the internal energy for the gas, after heating, will be equal to ${\text{U}}_2=\left(\text{N}-\text{n}\right)\left(\frac{5}{2}\text{R}\right)\text{T}+2\text{n}\left(\frac{3}{2}\text{R}\right)\text{T}=\frac{5}{2}\text{NRT}+\frac{1}{2}\text{nRT}$

Hence, the heat supplied = increase in internal energy

$=\left({\text{U}}_2-{\text{U}}_1\right)=\frac{1}{2}\text{nRT}$