Statement - I : When $\mu$ amount of an ideal gas undergoes adiabatic change from state $\left(P_1,V_1,T_1\right)$ to state $\left(P_2,V_2,T_2\right)$, then work done is $W=\frac{\mu R\left(T_2-T_1\right)}{1-\gamma }$, where $\gamma =\frac{C_P}{C_V}$ and $R=$ universal gas constant.

Statement - II : In the above case, when work is done on the gas, the temperature of the gas would rise.

A sample of an ideal gas is taken through the cyclic process $ABCA$ as shown in figure. It absorbs, $40 \mathrm{J}$ of heat during the part $AB$, no heat during $BC$ and rejects $60 \mathrm{J}$ of heat during $CA$. A work of $50 \mathrm{J}$ is done on the gas during the part $BC$. The internal energy of the gas at $A$ is $1560 \mathrm{J}$. The work done by the gas during the part $CA$ is