Question

What is the rate law for this reaction?

Express the rate law symbolically in terms of k , [A] , and [B] . [A]
(M) [B]
(M) Rate
(M/s)
1 0.20 0.030 1.4×10−3
2 0.20 0.060 2.9×10−3
3 0.40 0.030 5.8×10−3

Answer 1

The rate law for this reaction can be expressed as rate = k[A]²[B]°. The rate constant can be calculated using the given data. In this case, the rate constant is 0.0725 M⁻¹s⁻¹.

The rate law for this reaction can be expressed symbolically as rate = k[A]²[B]°. The rate law tells us how the rate of the reaction depends on the concentrations of the reactants. In this case, the reaction rate depends on the square of the concentration of reactant A and does not depend on the concentration of reactant B.

We can calculate the rate constant by using the data from any row of the table given. Let's use Experiment 2: 2.9×10−3 M/s = k(0.20 M)². Solving for k, we find that k = 0.0725 M⁻¹s⁻¹.