Question

he rate of reaction in terms of the "rate law expression" includes the rate constant (k), the concentration of the reactants, and the orders of the reaction with respect to the different reactants. Consider the following reaction: A+B→C+D The initial concentrations of the reactants A and B are 0.400 M and 0.290 M, respectively. The rate of reaction is 0.060 M⋅s−1, and the orders of the reaction, with respect to reactants A and B, are 1 and 2, respectively. Determine the rate constant (k) for the reaction using the rate law. Express your answer in M−2⋅s−1 to three significant figures. View Available Hint(s)

Answer 1

The rate constant for the given reaction is
`1.78 M^(-2)s^(-1)`.

Step-by-step explanation:

A + B → C + D

The initial concentrations of the reactants A = [A] = 0.400 M

The initial concentrations of the reactants B = [B] = 0.290 M

Order of reaction with respect to A = 1

Order of reaction with respect to B = 2

The rate of reaction = R = 0.060 M/s

The expression of the rate of the reaction will be given as:

`R=k[A]^1[B]^2`

`0.060 M/s=k[0.400 M]^1[0.290 M]^2`

`k=(0.060 M/s)/([0.400 M]^1[0.290 M]^2)=1.78 M^(-2)s^(-1)`

The rate constant for the given reaction is
`1.78 M^(-2)s^(-1)`.