Question

In a study of the reaction

A + B + C → products

at constant temperature, it was found that:

1. Holding [A] and [B] constant and halving the concentration of C causes the rate to proceed 2.828 times faster.

2. Holding [B] and [C] constant and doubling the concentration of A causes the reaction to proceed four times faster.

3. Doubling the concentrations of A, B, and C simultaneously, causes the reaction to proceed 1.414 times faster.

The experimental rate law is:

• A. Rate = k[A][B]²[C]^-1.5
• B. Rate = k[A]²[C]^-1.5
• C. Rate = k[A]²[B]^1.5
• D. Rate = k[A]²[B][C]^-0.5
• E. Rate = k[A][B]²[C]^-1

Answer 1