Which of the following is not true for the equilibrium reaction
`N_2(g)+O_2(g)hArr 2NO(g)`, `DeltaH=180kJmol^(-1)`

Options

A. The formation of `NO` is increased at higher temperature.
B. The volume change at constant pressure does not affect the equilibrium.
C. The pressure change at constant volume does not affect the equilibrium.
D. The formation of `NO` is decreased at higher temperature.

Answer

D

Explanation

It is endothermic (in the forward direction). Thus, a temperature increase favors the formation of NO. The pressure change at constant volume is possible by adding an inert gas. Similarly, the volume change at constant pressure can be achived by adding an inert gas. For this system, there is no effect of the addition of inert gas at constant volume or at constant pressure because `Delta n_(g)` is zero for this system, i.e., there is no change in the total number of moles of hases in a reaction.