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 $R$)

The combustion of one mole of benzene takes place at $298 \, K$ and $1 \, atm$. After combustion,$CO_{2(g)}$ and $H_2O_{(l)}$ are produced and $3267.0 \, kJ$ of heat is liberated. Calculate the standard enthalpy of formation,$\Delta_f H^{\ominus}$ of benzene. Standard enthalpies of formation of $CO_{2(g)}$ and $H_2O_{(l)}$ are $-393.5 \, kJ \, mol^{-1}$ and $-285.83 \, kJ \, mol^{-1}$ respectively.

Match List-$I$ with List-$II$

List-$I$	List-$II$
$A$. Spontaneous process	$I$. $\Delta H < 0$
$B$. Process with $\Delta P = 0; \Delta T = 0$	$II$. $\Delta G_{T, P} < 0$
$C$. $\Delta H_{reaction}$	$III$. Isothermal and isobaric process
$D$. Exothermic process	$IV$. [Bond energies of molecules in reactants] - [Bond energies of product molecules]

Choose the correct answer from the options given below:

When $3 \ mol$ of $Ar_{(g)}$ is supplied with $229 \ J$ of heat at constant pressure,the temperature of the sample increases by $2.55 \ K$. Calculate the molar heat capacity of the gas at constant volume.

Which of the following is (are) an endothermic reaction?

$\Delta H^o_f$ of water is $-285.5 \, kJ \, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3 \, kJ \, mol^{-1}$,$\Delta H^o_f$ of $OH^{-}$ ion will be.....$kJ \, mol^{-1}$