The reaction A + B „³ 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?
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?
To find the rate of the reaction, we need to use the rate law equation, which can be determined from the given order of reaction with respect to each reactant.
The rate law equation for a second order reaction in A and zero order in B is given by:
Rate = k * [A]^2 * [B]^0
Since the order of B is zero, it will not affect the rate of the reaction. We can simplify the rate law equation to:
Rate = k * [A]^2
Now, substitute the given values into the equation:
Rate = 0.012 M^-1 min^-1 * (0.125 M)^2
Rate = 0.012 M^-1 min^-1 * 0.015625 M^2
Rate = 0.0001875 M min^-1
Therefore, the rate of the reaction when [A] = 0.125 M and [B] = 0.435 M is 0.0001875 M min^-1.