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When a reversible reaction is at equilibrium, one of its products' concentration is decreased. The equilibrium state
- a)Shifts in the direction of backward reaction
- b)Shifts in the direction of forward reaction
- c)Is not affected
- d)Moves in either direction
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
When a reversible reaction is at equilibrium, one of its products conc...
According to Le Chatelier's principle, when a system at equilibrium is subjected to a change, the equilibrium shifts in the direction so as to undo the change. Therefore, if the concentration of product is decreased, the forward reaction takes place so as to increase the concentration.
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When a reversible reaction is at equilibrium, one of its products conc...
Explanation:
At equilibrium:
When a reversible reaction is at equilibrium, it means that the rates of the forward and backward reactions are equal. This implies that the concentrations of the reactants and products are constant over time.
Le Chatelier's principle:
Le Chatelier's principle states that if a system at equilibrium is subjected to a change, it will respond in such a way as to minimize the effect of that change and restore equilibrium. In the case of a reversible reaction, if the concentration of one of the products is decreased, the system will respond by shifting the equilibrium position to counteract this change.
Effect of decreasing product concentration:
When the concentration of one of the products in a reversible reaction is decreased, the equilibrium position will shift in the direction of the forward reaction. This means that the forward reaction will be favored, leading to an increase in the concentrations of the reactants and a decrease in the concentrations of the products.
Explanation in terms of reaction rates:
At equilibrium, the rate of the forward reaction is equal to the rate of the backward reaction. If the concentration of one of the products is decreased, the rate of the forward reaction will be greater than the rate of the backward reaction. This imbalance in reaction rates will cause the system to adjust by shifting the equilibrium position towards the forward reaction, in order to restore equilibrium.
Explanation in terms of equilibrium constant:
The equilibrium constant (K) is a measure of the extent to which a reaction proceeds towards the products. If the concentration of one of the products is decreased, the value of K will be greater than the current value at equilibrium. In order to increase the value of K and restore equilibrium, the system will shift towards the forward reaction, where more products are formed.
Therefore, when a reversible reaction is at equilibrium and one of its products' concentration is decreased, the equilibrium state will shift in the direction of the forward reaction (option B).
At equilibrium:
When a reversible reaction is at equilibrium, it means that the rates of the forward and backward reactions are equal. This implies that the concentrations of the reactants and products are constant over time.
Le Chatelier's principle:
Le Chatelier's principle states that if a system at equilibrium is subjected to a change, it will respond in such a way as to minimize the effect of that change and restore equilibrium. In the case of a reversible reaction, if the concentration of one of the products is decreased, the system will respond by shifting the equilibrium position to counteract this change.
Effect of decreasing product concentration:
When the concentration of one of the products in a reversible reaction is decreased, the equilibrium position will shift in the direction of the forward reaction. This means that the forward reaction will be favored, leading to an increase in the concentrations of the reactants and a decrease in the concentrations of the products.
Explanation in terms of reaction rates:
At equilibrium, the rate of the forward reaction is equal to the rate of the backward reaction. If the concentration of one of the products is decreased, the rate of the forward reaction will be greater than the rate of the backward reaction. This imbalance in reaction rates will cause the system to adjust by shifting the equilibrium position towards the forward reaction, in order to restore equilibrium.
Explanation in terms of equilibrium constant:
The equilibrium constant (K) is a measure of the extent to which a reaction proceeds towards the products. If the concentration of one of the products is decreased, the value of K will be greater than the current value at equilibrium. In order to increase the value of K and restore equilibrium, the system will shift towards the forward reaction, where more products are formed.
Therefore, when a reversible reaction is at equilibrium and one of its products' concentration is decreased, the equilibrium state will shift in the direction of the forward reaction (option B).
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When a reversible reaction is at equilibrium, one of its products concentration is decreased. The equilibrium statea)Shifts in the direction of backward reactionb)Shifts in the direction of forward reactionc)Is not affectedd)Moves in either directionCorrect answer is option 'B'. Can you explain this answer?
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