In aqueous solution, iodine reacts with acetone as represented by the following

Question

In aqueous solution, iodine reacts with acetone as represented by the following equation: I2(aq) + CH3COCH3(aq) CH3COCH2I(aq) + H+(aq) + I–(aq) The experimental rate law is Rate = k[H+][CH3COCH3]. According to the information above, an increase in the hydrogen ion concentration has what effect on the reaction?

A. It decreases the rate of the reaction.

B. It decreases the value of the equilibrium constant.

C. It increases the rate of the reaction.

D. It does not affect the rate of the reaction.

E. It increases the value of the equilibrium constant.

Explanation / Answer

If rate depends directly on:

Rate = k[H+][CH3COCH3]

then

increasing [H+] will increase the Rate proportionally

Since [H+] is a reactant required for reaciton, and the rate law allow sus understand that the more [H+] present, the more it reacts (i.e. faster, due to collision theory)

Therefore, the best answer is;

C. It increases the rate of the reaction.

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