Question

${\mathrm{N}}_2+{\mathrm{O}}_2\rightleftharpoons 2\mathrm{NO}+\mathrm{Heat}$.

In the above given chemical reaction, which of the following conditions is suitable to get a good yield of $\mathrm{NO}$?

• A. Increase in pressure
• B. Decrease in pressure
• C. Increase in temperature
• D. Decrease in temperature

Answer 1

The correct option is C

Increase in temperature

Explanation for correct option:

(c) Increase in temperature

Le Chatelier's principle:

• The equilibrium law, also known as Le Chatelier's principle, is used to forecast the effect of a change in components on a thermodynamic system in chemical equilibrium.
• It is claimed that equilibrium may alter the forward and backward responses in such a way that the changes influencing the equilibrium are negated.
• According to the Le Chatelier Principle, a change in temperature, pressure, or reactant concentration in an equilibrium system will cause the equilibrium to shift into a new equilibrium, negating the impact of the change.
• Adding or withdrawing heat alters the equilibrium in the event of temperature change.
• As given in the question:

$\underset{\mathrm{Nitrogen}\mathrm{gas}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{Oxygen}\mathrm{gas}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\rightleftharpoons \underset{\mathrm{Nitric}\mathrm{oxide}}{2\mathrm{NO}\left(\mathrm{g}\right)}+\mathrm{Heat}$

• The reaction is endothermic in the forward direction, which increases in temperature and favors the formation of Nitric oxide($\mathrm{NO}$).
• So, the correct option is (c).