Question

According to Le Chatelier's principle, in the reaction \( \text{CO}(g) + 3\text{H}_2(g) \rightleftharpoons \text{CH}_4(g) + \text{H}_2\text{O}(g) \), the formation of methane is favoured by

• A. increasing the concentration of CO
• B. increasing the concentration of H_2O
• C. decreasing the concentration of CH_4
• D. decreasing the concentration of H_2

Hint:

Le Chatelier’s principle helps predict the direction of equilibrium shifts in response to changes in concentration, pressure, or temperature.

Answer 1

The Correct Option is D

Le Chatelier’s principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will shift to counteract that change. In this case:
- Increasing the concentration of CO will shift the reaction to the right, favouring the formation of CH_4.
- Decreasing the concentration of CH_4 will also shift the equilibrium to the right to produce more CH_4.
Thus, increasing the concentration of CO and decreasing the concentration of CH_4 favours the formation of methane.