In an adiabatic process, $90 \mathrm{J}$ of work is done on the gas. The change in internal energy of the gas 

One mole of diatomic ideal gas undergoes a cyclic process $ABC$ as shown in the figure. The process $BC$ is adiabatic. The temperatures at $A, B$ and $C$ are $400 \mathrm{K}, 800 \mathrm{K}$ and $600 \mathrm{K}$, respectively. Choose the correct statement.

The internal energy change in a system that has absorbed $2 \mathrm{kcal}$ of heat and done $500 \mathrm{J}$ of work is similar, 

If $Q, E \mathrm{and} W$ denote respectively the heat added, change in internal energy and the work done in a closed cycle process, then,

$110 \mathrm{J}$ of heat is added to a gaseous system, whose internal energy change is $40 \mathrm{J}$, then the amount of external work done is,

When heat energy of $1500 \mathrm{J}$ is supplied to a gas at constant pressure $2.1\times {10}^5 \mathrm{N} {\mathrm{m}}^{-2},$ there is an increase in its volume equal to $2.5\times {10}^{-3} {\mathrm{m}}^3$. The increase in internal energy of the gas in $\mathrm{Joules}$  is

During an isothermal expansion, a confined ideal gas does $-150 \mathrm{J}$ of work against its surrounding. This implies that,

If the amount of heat given to a system is $35 \mathrm{J}$ and the amount of work done on the system is $15 \mathrm{J},$ then the change in internal energy of the system is,