In aqueous solution, iodine reacts with acetone as represented by the following stoichiometric equation:
I2 + CH3COCH3---> CH3COCH2I + H+ + Iâ?"
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?
It decreases the rate of the reaction.
It increases the rate of the reaction.
It does not affect the rate of the reaction.
It decreases the value of the equilibrium constant.
It increases the value of the equilibrium constant.
In this solution the question of equilibrium is considered. Specifically, what happens to the rate of a reaction when you add a certain component to the system, given the rate law?