For a substance,the molar heat capacity at constant $P$ is given by:

One mole of a gas occupying $3 \ L$ volume is expanded against a constant external pressure of $1 \ bar$ to a volume of $15 \ L$. Calculate the work done by the system.

The enthalpy of a reaction at $273 \, K$ is $-3.57 \, kJ$. If $\Delta C_p = 0$,what will be the enthalpy of the reaction at $373 \, K$?

What is the work done when $2 \text{ mole}$ of an ideal gas are expanded isothermally and reversibly from $5 \text{ m}^{3}$ to $10 \text{ m}^{3}$ at $300 \text{ K}$ (in $\text{ kJ}$)? $(R=8.314 \text{ J K}^{-1} \text{ mol}^{-1})$

Explain: $\Delta H = q_{p}$

The magnitude of work done by a gas that undergoes a reversible expansion along the path $ABC$ shown in the figure is .............. $Joule$.