Which statement correctly pairs the order of a reaction with the units for the rate constant?

A. third order; s/M
B. zero order; 1/(M2)
C. second order; 1/(M•s)
D. first order; 1/M

second order; 1/(M•s)

To determine the correct pairing of the order of a reaction with the units for the rate constant, we need to understand the relationship between the rate equation and the order of the reaction.

The rate equation generally takes the form:

Rate = k[A]^m[B]^n

where [A] and [B] represent the concentrations of species A and B, and m and n are the reaction orders for A and B, respectively. The overall order of the reaction is the sum of the reaction orders for all species involved.

Now, let's consider each option and determine the correct pairing:

A. third order; s/M
This means the overall reaction order is 3. The units for the rate constant (k) in this case would be s/M, since the rate equation can be written as Rate = k[A]^3.

B. zero order; 1/(M^2)
This means the overall reaction order is 0. The units for the rate constant (k) in this case would be 1/(M^2), since the rate equation can be written as Rate = k[A]^0 = k.

C. second order; 1/(M•s)
This means the overall reaction order is 2. The units for the rate constant (k) in this case would be 1/(M•s), since the rate equation can be written as Rate = k[A]^2.

D. first order; 1/M
This means the overall reaction order is 1. The units for the rate constant (k) in this case would be 1/M, since the rate equation can be written as Rate = k[A].

Based on these explanations, the correct pairing of the order of a reaction with the units for the rate constant is:
C. second order; 1/(M•s)

https://www.google.com/search?q=units+for+order+of+reaction&ie=utf-8&oe=utf-8

so is it d ?