In an adiabatic expansion of 0.5 mole of an ideal diatomic gas, temperature changes from 32ºC to 20ºC. The change in internal energy of the gas is 

The following are the P-V diagrams for cyclic processes for a gas. In which of these processes heat is released by the gas ?

An ideal gas is taken through the cycle $A\to B\to C\to A,$ as shown in the figure. If the net heat supplied to the gas in the cycle is $5 \mathrm{J}$, the work done by the gas in the process $C\to A$ is

One mole of a monatomic ideal gas is taken through a cycle $ABCDA$ as shown in the $P-V$ diagram. Column-II gives the characteristics involved in the cycle. Match them with each of the processes given in Column-I.

Three processes form a thermodynamic cycle as shown on $P-V$ diagram for an ideal gas. Process $1\to 2$ takes place at constant temperature ($300 \mathrm{K}$), Process $2\to 3$ takes place at constant volume, During this process $40 \mathrm{J}$ of heat leaves the system. Process $3\to 1$ is adiabatic and temperature $T_2,\text{ is} 275 \mathrm{K}$. Work done by the gas during the process $3\to 1$ is