An ideal gas expands isothermally from $10^{-3} \; m^{3}$ to $10^{-2} \; m^{3}$ at $300 \; K$ against a constant external pressure of $10^{5} \; Nm^{-2}$. The work done on the gas is:

If $0.75 \ mol$ of an ideal gas expands isothermally at $27 \ ^{\circ}C$ from $15 \ L$ to $25 \ L$,the maximum work obtained is ...... $J$. (in $.5$)

In an endothermic reaction,the value of $\Delta H$ is

The internal energy of a substance $U$ is related to temperature $T$ in which of the following ways?

For the reaction of nitrogen with hydrogen to form ammonia,$\Delta H^o = -92.2 \ kJ/mol$. If the reaction is carried out at a constant pressure of $20.0 \ atm$ and a volume change of $-1.16 \ L$,calculate the change in internal energy $(\Delta U)$ in $kJ$.

$A$ sample of $1.0 \ mol$ of a monoatomic ideal gas is taken through a cyclic process of expansion and compression as shown in the figure. What will be the value of $\Delta H$ for the cycle as a whole?