if the concentrated of A is reduced
if the concentrated of B is reduced
if the concentrated of C is reduced
if the concentration of C is increased
if D is continuously removed from the reaction mixture
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Discussions (5)
A + B ⇌ C + D
This equation shows a reversible reaction that can go in both directions—forward (making products C and D) and backward (making reactants A and B).
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What is Le Chatelier’s Principle?
Le Chatelier’s Principle says:
> If a system at equilibrium is disturbed, the system will shift in a direction that counteracts the disturbance and tries to restore equilibrium.
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Let’s look at each option in your question:
A. If the concentration of A is reduced:
The system loses some reactant.
It shifts left to make more A and B.
So, less D will be formed.
→ Not correct.
B. If the concentration of B is reduced:
Same idea: removing a reactant shifts the reaction left.
This also means less D is produced.
→ Not correct.
C. If the concentration of C is reduced:
Removing C (a product) causes the reaction to shift right, to replace the lost product.
This will lead to more D being formed.
→ This is technically true—but not the best choice, because the effect might not be as strong or continuous.
D. If the concentration of C is increased:
Adding a product pushes the reaction left to reduce C.
This will result in less D.
→ Not correct.
E. If D is continuously removed from the reaction mixture:
Removing D means the system keeps trying to make up for the loss by shifting right.
This constantly produces more D.
→ This is the best and most effective option.
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Why E is the BEST answer
Unlike a one-time change (like removing some C), continuously removing D keeps the system pushed to the right, keeping the reaction going and producing more and more D until the reactants run out or other limits are reached.
