Question
Define: $(a)$ Reversible process $(b)$ Standard enthalpy of combustion.
Calculate the enthalpy change for the reaction: $N _{2( g )}+3 H _{2( g )} \longrightarrow 2 NH _{3( g )}$.
The bond enthalpies are:
Calculate the enthalpy change for the reaction: $N _{2( g )}+3 H _{2( g )} \longrightarrow 2 NH _{3( g )}$.
The bond enthalpies are:
| Bond | $N \equiv N$ | $H-H$ | $N-H$ |
| $\Delta H ^0$ in $kJ mol ^{-1}$ | $946$ | $435$ | $389$ |