Nitric acid is made industrially by the oxidation of ammonia. The overall equation for the process is shown.
equation 1: NH$_3$ + 2O$_2$ → HNO$_3$ + H$_2$O
The process happens in three stages. The equations and enthalpy changes for these stages are given.
stage 1: 4NH$_3$ + 5O$_2$ → 4NO + 6H$_2$O ΔH = -904kJ mol$^{ - 1}$
stage 2: 2NO + O$_2$ → 2NO$_2$ ΔH = -114kJ mol$^{ - 1}$
stage 3: 4NO$_2$ + O$_2$ + 2H$_2$O → 4HNO$_3$ ΔH = -348kJ$ $mol$^{ - 1}$
What is the enthalpy change of the process shown in equation 1?
1 )
−1480 kJ mol$^{−1}$
−370 kJ mol$^{−1}$
3 )
−341.5 kJ mol$^{−1}$
4 )
+82 kJ mol$^{−1}$
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