The equation given above is exothermic (ΔH is negative), 92.4 kJ of energy per mole of N_{2}(g) is released.

This equation can be reversed to show the decomposition of ammonia into nitrogen and hydrogen gas. This will require an input of 92.4 kJ of energy per mole of nitrogen gas, that is, the reaction will be endothermic.

92.4 kJ of energy is released for every 1 mole of N_{2}(g)

92.4 kJ of energy is released for every 3 moles of H_{2}(g)

92.4 kJ of energy is released for every 2 moles of NH_{3}(g) produced.

How much energy is released if only 1 mole of ammonia (NH_{3}) gas is produced?

92.4 kJ of energy is released in the production of 2 moles of ammonia gas
Half as much energy will be released if only half the amount of ammonia gas is produced
½ x 92.4 = 46.2 kJ of energy will be released in the production of 1 mole of ammonia.

How much energy is released if 10 moles of nitrogen (N_{2}) gas and 30 moles of hydrogen (H_{2}) gas is used in the reaction?

92.4 kJ of energy is released for every 1 mole of N_{2}(g)
10 times as much energy will be released if 10 times the amount of reactants are used
10 x 92.4 = 924kJ of energy will be released

How much energy is released if 5 moles of hydrogen (H_{2}) gas and ^{5}/_{3} mole of nitrogen (N_{2}) gas is used in the reaction?

92.4 kJ of energy is released for every 3 moles of H_{2}(g)
The amount of energy released for every mole of hydrogen gas used = 92.4 ÷ 3 = 30.8 kJ mol^{-1} of H_{2}(g)
The amount of energy released for 5 moles of hydrogen gas = 5 x 30.8 = 154 kJ