Question:
Consider the water gas equilibrium reaction,
\[
C(s) + H_2O(g) \rightleftharpoons CO(g) + H_2(g)
\]
Which of the following statements is true at equilibrium?
Consider the water gas equilibrium reaction,
\[
C(s) + H_2O(g) \rightleftharpoons CO(g) + H_2(g)
\]
Which of the following statements is true at equilibrium?
Show Hint
Le Chatelier's principle states that a system at equilibrium will adjust to counteract changes in concentration, pressure, or temperature.
Updated On: Jan 12, 2026
- If the amount of \( C(s) \) is increased, less water would be formed
- If the amount of \( C(s) \) is increased, more CO and \( H_2 \) would be formed
- If the pressure on the system is increased by halving the volume, more water would be formed
- If the pressure on the system is increased by halving the volume, more CO and \( H_2 \) would be formed
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The Correct Option is B
Solution and Explanation
Increasing the amount of carbon shifts the equilibrium towards the products, increasing the concentrations of CO and \( H_2 \) according to Le Chatelier's principle.
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