For the Reaction Represented Below, the Experimental Rate Law Is $\rarr$

For the reaction represented below, the experimental rate law is given by rate = k [(CH₃) ₃CCl]. (CH₃) ₃CCl(aq) + OH^- $\rarr$ (CH₃) ₃COH(aq) + Cl^-
If some solid sodium hydroxide were added to a solution in which [(CH₃) ₃CCl] = 0.01 M and
[NaOH] = 0.10 M, which of the following would be true? (Assume the temperature and volume remain constant.)

A) Both the reaction rate and k would increase.
B) Both the reaction rate and k would decrease.
C) Both the reaction rate and k would remain the same.
D) The reaction rate would increase but k would remain the same.
E) The reaction rate would decrease but k would remain the same.

Correct Answer:

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