Consider the equilibrium $\mathrm{CO}(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons…

Consider the equilibrium
$\mathrm{CO}(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{~g})$
If the pressure applied over the system increases by two fold at constant temperature then
(A) Concentration of reactants and products increases.
(B) Equilibrium will shift in forward direction.
(C) Equilibrium constant increases since concentration of products increases.
(D) Equilibrium constant remains unchanged as concentration of reactants and products remain same.
Choose the correct answer from the options given below :
  1. (A), (B) and (C) only
  2. (A) and (B) only
  3. (A), (B) and (D) only
  4. (B) and (C) only

Solution

$\begin{aligned} & \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_2 \rightleftharpoons \mathrm{CH}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \\ & \Delta \mathrm{n}_{\mathrm{g}}=-2\end{aligned}$
If pressure of system increases then according to Le-Chatelier's principle reaction will move in forward direction.
Concentration of reactant and products both increases but concentration of product increases more.

Asked in: JEE Main 2025 (29 Jan Shift 2)

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