Consider the reaction cl2 (g) + i2 (g) 2 icl (g), which is endothermic as written. what would be the effect on the equilibrium position of removing cl2 (g) ? 1. reaction would go to the left, making more "reactants" 2. no change on the equilibrium position 3. reaction would go to the right, making more "reactants" 4. reaction would go to the left, making more "products" 5. reaction would go to the right, making more "products"

Question

Chemistry

Watson

14 August, 11:32

Consider the reaction cl2 (g) + i2 (g) 2 icl (g), which is endothermic as written. what would be the effect on the equilibrium position of removing cl2 (g) ? 1. reaction would go to the left, making more "reactants" 2. no change on the equilibrium position 3. reaction would go to the right, making more "reactants" 4. reaction would go to the left, making more "products" 5. reaction would go to the right, making more "products"

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Ali Robbins · Answer 1

1. The position of equilibrium would shift to the left, making more reactants.

Cl₂ (g) + I₂ (g) + heat ⇌ 2ICl (g)

Le Châtelier's Principle states that, if you add a stress to a system at equilibrium, the system will respond in a direction that will remove the stress.

Here, the stress is the removal of Cl₂. The system will respond by generating more Cl₂ to replace what was removed.

The position of equilibriumwill move to the left.