The standard enthalpy of neutralization is \(-57.3 \mathrm{~K}{\mathrm{J}}~ \mathrm{mol}^{-1}\)as:
\(\small{\underset{\text{strong acid}}{\mathrm{HCl_{(aq)}}}+\underset{\text{strong base}}{\mathrm{NaOH_{(aq)}}}\rightarrow\mathrm{NaCl_{(aq)}+H_2O(l),\Delta H=-57.3~KJ mol^{-1}}} \)
The enthalpy of neutralization of \(0.25 \mathrm{~mol}\) of HCI by \(0.25 \mathrm{~mol}\) of \(\mathrm{NaOH}\) is :
1. \(-57.3~ \mathrm{kJ} ~\mathrm{mol}^{-1}\)
2. \(-28.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3. \(-14.32 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4. \(+57.3~ \mathrm{kJ}~ \mathrm{mol}^{-1}\)