Question

How does [B] change when D is added to the following reaction at equilibrium? 2 A(g)...

How does [B] change when D is added to the following reaction at equilibrium?
2 A(g) + B(g) ↔ 2 C(g) + D(s)

How does [B] change when D is added to the following reaction at equilibrium?
2 A(g) + B(g) ↔ 2 C(g) + D(s)

[B] will not change.
Cannot be predicted.
[B] will increase.
[B] will decrease.
Science   Chemistry   
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Homework Answers

Answer #1

According to the Le-Charterlier's principle,If the concentration of reactants is increased or product is removed , the reaction will take place in the forward direction.

If the concentration of products is increased or reactants is removed , the reaction will take place in the backward direction.

2 A(g) + B(g) ↔ 2 C(g) + D(s)

By addition of D( which is a product) the concentration of product is increasing so the backward reaction takes place so that the concentration of B increases.

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