One mole of a gas absorbs $200 \ J$ of heat at constant volume. Its temperature increases from $298 \ K$ to $308 \ K$. The change in its internal energy is ....... Joules.

At $300 \ K$,the enthalpy change for the reaction $C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(l)$ is $-2800 \ kJ \ mol^{-1}$. Calculate the internal energy change $(\Delta U)$ for the reaction at the same temperature.

$A$ system does $200 \, J$ of work and at the same time absorbs $150 \, J$ of heat. The magnitude of the change in internal energy is $..... \, J.$ (Nearest integer)

$C_2H_5OH(l) + 3O_2(g) \rightarrow 2CO_2(g) + 3H_2O(l)$. The enthalpy change $(\Delta H)$ for the above reaction at $27^{\circ}C$ is $-1366.5 \text{ kJ mol}^{-1}$. Calculate the internal energy change $(\Delta U)$ for the same reaction at this temperature.

The correct relationship is

Work done in vaporisation of one mole of water at $373 \ K$ and the pressure of $1 \ atm$ is approximately (for ideal gas)......$J$