Comment on the thermodynamic stability of NO(g), given N 2 (g) + O 2 (g) → NO(g); = 90 kJ mol –1 NO(g) + O 2 (g) → NO 2 (g): = –74 kJ mol –1

Question

Philoid · Accepted Answer

The first reaction is endothermic. It consumes or absorbs energy to form products. So, NO has more energy than its reactants. Hence, NO is unstable.

In the second reaction, it reacts with oxygen to form NO₂, and gives off energy. It’s an exothermic reaction. So, NO₂ has less energy than its reactants, and is stable. It is stabilised with minimum energy.

Hence unstable NO gets converted into stable NO₂.

Comment on the thermodynamic stability of NO(g), givenN2(g) +O2(g) → NO(g); = 90 kJ mol–1NO(g) +O2(g) → NO2(g): = –74 kJ mol–1

Comment on the thermodynamic stability of NO(g), given
N₂(g) +O₂(g) → NO(g); = 90 kJ mol^–1

NO(g) +O₂(g) → NO₂(g): = –74 kJ mol^–1