Three moles of an ideal gas are expanded isothermally from a volume of $300 \ cm^3$ to $2.5 \ L$ at $300 \ K$ against a constant external pressure of $1.9 \ atm$. The work done in joules is:

The value of $\Delta H$ for cooling $2 \ mol$ of an ideal monoatomic gas from $225^{\circ} C$ to $125^{\circ} C$ at constant pressure will be [given $C_{p} = \frac{5}{2} R$]. (in $R$)

$20.0 \ dm^{3}$ of an ideal gas '$X$' at $600 \ K$ and $0.5 \ MPa$ undergoes isothermal reversible expansion until the pressure of the gas is $0.2 \ MPa$. Which of the following options is correct? (Given: $\log\,2=0.3010$ and $\log\,5=0.6989$)

The molar heat of neutralization of $NaOH$ with $HCl$ in comparison to that of $KOH$ with $HNO_3$ is:

Which of the following statements or relationships is not correct in thermodynamic changes?

For the hypothetical reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$
$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.
If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$