An ideal gas expands by performing $200 \ J$ of work,during this internal energy increases by $432 \ J$. What is the enthalpy change (in $J$)?

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J/K)$ .....$K$

In a particular reaction, $4 \text{ kJ}$ of heat is released by the system and $12 \text{ kJ}$ of work is done on the system. Calculate the $\Delta H$ and $\Delta U$.

In a process,the work done by the system is equal to the change in its internal energy. Then the process will be ...........

What is the change in internal energy if a system gains $x \ J$ of heat and $y \ J$ of work is done on it?

If $2 \text{ mole}$ of an ideal gas expand isothermally and reversibly at $27^{\circ}C$ from $1 \text{ dm}^3$ to $1 \text{ m}^3$, calculate the work done. [$R = 8.314 \text{ J K}^{-1} \text{mol}^{-1}$] (in $\text{ kJ}$)