Question

$3H_2\left(g\right)+N_2\left(g\right)\rightleftharpoons 2{NH}_3\left(g\right)$ + heat energy

Which of the following conditions would shift the equilibrium of this reaction so that the formation of ammonia is favored?

• A. Increasing the pressure of the reaction
• B. Heating the reaction
• C. Removing hydrogen gas from the reaction
• D. Adding more ammonia to the reaction
• E. Removing nitrogen gas from the reaction

Answer 1

The correct option is A Increasing the pressure of the reaction

This is a gaseous reaction where reactant and products are gas, here on increasing the pressure, the reaction will shift to that direction where the effect of increasing of pressure could be nullified.
Hence , reaction goes to that direction where the number of moles are less in number,
In this reaction, the number of moles are less in the product side, where there is formation of the $N{H}_3$ hence the formation of $N{H}_3$ is favoured by the increase in pressure.
$3H_2\left(g\right)+N_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$