Find the enthalpy of neutralisation in $kJ/mol$ for the reaction between $NH_4OH$ and $HCN$ in aqueous solution,given that the enthalpies of ionisation of $NH_4OH$ and $HCN$ are $7 \ kJ/mol$ and $8 \ kJ/mol$ respectively,and the enthalpy of neutralisation of a strong acid and a strong base is $-57.3 \ kJ/mol$.
- A$-42.3$
- B$-57.3$
- C$-72.3$
- D$+42.3$
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$A$. Isothermal process $i$. $q = \Delta U$ $B$. Adiabatic process $ii$. $W = - P \times \Delta V$ $C$. Isobaric process $iii$. $W = \Delta U$ $D$. Isochoric process $iv$. $W = - nRT \ln \left(\frac{v_f}{v_i}\right)$
| $A$. Isothermal process | $i$. $q = \Delta U$ |
| $B$. Adiabatic process | $ii$. $W = - P \times \Delta V$ |
| $C$. Isobaric process | $iii$. $W = \Delta U$ |
| $D$. Isochoric process | $iv$. $W = - nRT \ln \left(\frac{v_f}{v_i}\right)$ |
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View SolutionThe heat of combustion of carbon to $CO_2$ is $-393.5 \text{ kJ/mol}$. The heat released upon formation of $35.2 \text{ g}$ of $CO_2$ from carbon and oxygen gas is
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