Question

At 1000 K, the equilibrium constant for the reaction
\(\text{CO}_2(\text{g}) + \text{H}_2(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + \text{H}_2\text{O}(\text{g})\) is 0.53. In a one litre vessel, at equilibrium the mixture contains 0.25 mole of CO, 0.5 mole of \(\text{CO}_2\), 0.6 mole of \(\text{H}_2\) and \(x\) moles of \(\text{H}_2\text{O}\). The value of \(x\) is

• A. 0.563
• B. 0.363
• C. 0.636
• D. 0.736

Hint:

For reactions where \(\Delta n_g = 0\) (equal moles of gas on both sides), the equilibrium constant expression depends only on the moles, and the volume term cancels out.

Answer 1

The Correct Option is C