The heat of neutralisation of an acid by a base is highest when:

Given $C + O_2 \rightarrow CO_2$ : $\Delta H = -x \ kJ$ and $2CO + O_2 \rightarrow 2CO_2$ : $\Delta H^\circ = -y \ kJ$,find the enthalpy of formation of carbon monoxide.

The enthalpy change for the reaction,$C_{2}H_{6(g)} \to 2C_{(g)} + 6H_{(g)}$ is $X \ kJ$. The bond energy of $C-H$ bond is :-

Which of the following compounds has a standard molar enthalpy of formation equal to zero at $298 \ K$?

The heat of neutralisation of a strong acid and a strong alkali is $57.0 \, kJ \, mol^{-1}$. The heat released when $0.5 \, mole$ of $HNO_3$ solution is mixed with $0.2 \, mole$ of $KOH$ is $...... \, kJ$.

$S_{\text{(rhombic)}} + O_{2(g)} \rightarrow SO_{2(g)}; \Delta H = -297.5 \, kJ$
$S_{\text{(monoclinic)}} + O_{2(g)} \rightarrow SO_{2(g)}; \Delta H = -300 \, kJ$
From the given data,which of the following statements is correct?