Consider the gas-phase equilibrium system represented by the equation:
$2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g)$
Given that the forward reaction is endothermic, which of the following changes will decrease amount of $H_{2} O ?$

removing more oxygen

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increasing the temperature at constant pressure

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Adding a solid phase catalyst

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Both a and b

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Solution

The correct option is D Both a and b
According to Le chatelier's principle, for an endothermic reaction, increasing the temperature will shift the equilibrium to the right, while decreasing the temperature will shift the equilibrium to the left. Removing the oxygen, will decrease the reaction quotient and hence forward reaction is more favoured. Catalyst does not shift the equilibrium. It only helps to attain the equilibrium faster.

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