A change in concentration increases the rate of a certain forward reaction more

Question

A change in concentration increases the rate of a certain forward reaction more than that of the reverse reaction. What is the effect on the equilibrium constant and the concentrations of reactants and products at equilibrium?

The product concentration(s) will decrease. The reactant concentration(s) will decrease. The equilibrium constant will not change.

The product concentration(s) will increase. The reactant concentration(s) will decrease. The equilibrium constant will not change.

The product concentration(s) will increase. The reactant concentration(s) will decrease. The equilibrium constant will increase.

The product concentration(s) will decrease. The reactant concentration(s) will increase. The equilibrium constant will decrease.

The product concentration(s) will decrease. The reactant concentration(s) will decrease. The equilibrium constant will not change.

The product concentration(s) will increase. The reactant concentration(s) will decrease. The equilibrium constant will not change.

The product concentration(s) will increase. The reactant concentration(s) will decrease. The equilibrium constant will increase.

The product concentration(s) will decrease. The reactant concentration(s) will increase. The equilibrium constant will decrease.

Explanation / Answer

A forward reaction is :   Reactants ----------> Products

The increase in the rate of the forward reaction will increase the concentrations of products and will decrease the concentarions of the reactants.

Equilibrium constant ( Ka) = [Products ] / [Reactants]

For this reason, the equilibrium constant with increase because concentrations of products will increase.

Therefore, third choice is the right answer.

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