The enthalpies of formation of gaseous $N_2O$ and $NO$ at $298 \ K$ are $82.0$ and $90.0 \ kJ \ mol^{-1}$ respectively. The enthalpy change of the reaction $N_2O_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow 2 NO_{(g)}$ is

The amount of heat released when $20 \ mL$ of $0.5 \ M$ $NaOH$ is mixed with $100 \ mL$ of $0.1 \ M$ $HCl$ is $x \ kJ$. The heat of neutralization is:

$C_{(s)} + 2 H_{2(g)} \rightarrow CH_{4(g)}$; $\Delta H = -74.8 \ kJ \ mol^{-1}$
Which of the following diagrams gives an accurate representation of the above reaction?
[$R \rightarrow$ reactants; $P \rightarrow$ products]

Match the following:

List-$I$	List-$II$
$(A) \Delta U = W_{ad}$	$I.$ Isothermal reversible expansion
$(B) \Delta U = q - W$	$II.$ Wall is adiabatic
$(C) \Delta U = -q$	$III.$ Thermally conducting walls
$(D) \Delta U = 0$	$IV.$ Isolated system
	$V.$ Closed system

The correct answer is

Given below are two statements:
Statement $I$: For an ideal gas, heat capacity at constant volume is always greater than the heat capacity at constant pressure.
Statement $II$: In a constant volume process, no work is produced and all the heat withdrawn goes into the chaotic motion and is reflected by a temperature increase of the ideal gas.

For the complete combustion of methanol
$CH_3OH_{(l)} + \frac{3}{2} O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O_{(l)}$
the amount of heat produced as measured by a bomb calorimeter is $726 \ kJ \ mol^{-1}$ at $27^{\circ}C$. The enthalpy of combustion for the reaction is $-x \ kJ \ mol^{-1}$,where $x$ is $.....$ (Nearest integer).
(Given: $R = 8.3 \ J \ K^{-1} \ mol^{-1}$)