Comment on the thermodynamic stability of NO(g), given, (i) 1/2 N_(2)(g) + 1/2O_(2)(g) to NO(g) Delta_(r)H^(@) = 90 kJ mol^(-1) (ii)NO(g) + 1/2 O_(2)(g) to NO_(2)(g) Delta_(r)H^(@) = -74 kJ mol^(-1).

Comment on the thermodynamic stability of NO(g), given, (i) 1/2 N_(2)

1.	Comment on the thermodynamic stability of NO(g), given, (i) 1/2 N_(2)(g) + 1/2O_(2)(g) to NO(g) Delta_(r)H^(@) = 90 kJ mol^(-1) (ii)NO(g) + 1/2 O_(2)(g) to NO_(2)(g) Delta_(r)H^(@) = -74 kJ mol^(-1).
Answer» Solution :Since `Delta_(r)H^(@)` is + ve i.e., ENTHALPY of formation of NO is positive so NO(G) is unstable.But `NO_(2)(g)` is formed because ENERGY is released.