The reaction A + B --> C + D is second order in A and zero order in B. The value of k is 0.012 M-1 min-1. What is the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M?
r= k(t)*.125^2 * .435^0
To find the rate of the reaction, we can use the rate equation for a second-order reaction:
rate = k * [A]^2
Given that the reaction is second order in A, we have [A]^2 in the rate equation. We also know that the reaction is zero order in B, meaning the concentration of B does not affect the rate of the reaction.
Plugging in the given values:
rate = k * [A]^2
= 0.012 M^-1 min^-1 * (0.125 M)^2
First, we square the concentration of A:
[A]^2 = (0.125 M)^2 = 0.015625 M^2
Now, substitute this value into the rate equation:
rate = 0.012 M^-1 min^-1 * 0.015625 M^2
Performing the multiplication:
rate = 0.0001875 M min^-1
Therefore, the rate of this reaction when [A] = 0.125 M and [B] = 0.435 M is 0.0001875 M min^-1.