Match the following items in List-$I$ with their corresponding expressions in List-$II$.

List-$I$	List-$II$
$A$. At constant volume the change in internal energy of a system	$I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$
$B$. Isothermal irreversible change	$II$. $W_{adiabatic} = \Delta U$
$C$. Isothermal reversible change	$III$. $q_V = \Delta U$
$D$. Adiabatic change	$IV$. $W = -p_{ex} (V_f - V_i)$
	$V$. $\Delta U = \Delta H - \Delta nRT$

The heat associated with the combustion of liquid benzene at constant volume is $-3268 \ kJ \ mol^{-1}$. Calculate the change in enthalpy when this reaction occurs at $300 \ K$ $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$.

The work done during the combustion of $9 \times 10^{-2} \ kg$ of ethane,$C_2H_{6(g)}$ at $300 \ K$ is (Given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$,atomic mass $C = 12$,$H = 1$). (in $kJ$)

For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$ at $977 \ ^oC$,given $\Delta H = 176 \ kJ \ mol^{-1}$,the value of $\Delta E$ is ............. $kJ$.

How much heat in $KJ$ is released during the combustion of $112 \ L$ of water gas at $S.T.P.$? (Water gas is an equimolar mixture of $H_2$ and $CO$)
$H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(g)}; \Delta H = -241.8 \ KJ$
$CO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{2(g)}; \Delta H = -283 \ KJ$

$2 \ mol$ of $Hg_{(g)}$ is combusted in a fixed volume bomb calorimeter with excess of $O_2$ at $298 \ K$ and $1 \ atm$ into $HgO_{(s)}$. During the reaction,temperature increases from $298.0 \ K$ to $312.8 \ K$. If heat capacity of the bomb calorimeter and enthalpy of formation of $Hg_{(g)}$ are $20.00 \ kJ \ K^{-1}$ and $61.32 \ kJ \ mol^{-1}$ at $298 \ K$,respectively,the calculated standard molar enthalpy of formation of $HgO_{(s)}$ at $298 \ K$ is $X \ kJ \ mol^{-1}$. The value of $|X|$ is. . . . . [Given : Gas constant $R = 8.3 \ J \ K^{-1} \ mol^{-1}$]