Question

the zero order reaction a → products takes 63.5 minutes for the concentration of a to decrease from 0.970 m to 0.209 m. what is the value of k for this reaction?

Answer 1

To find the value of k for the zero-order reaction a → products, substitute the given concentrations and time into the integrated rate law equation. After simplifying the equation, you will find the value of k to be approximately 0.012 M/min.

Step-by-step explanation:

To find the value of k for the zero-order reaction, we can use the integrated rate law for a zeroth-order reaction, which is given by [A] = [A]o - kt. In this case, the initial concentration of A is 0.970 M and it decreases to 0.209 M over a time of 63.5 minutes. We can substitute these values into the equation to solve for k:

0.209 M = 0.970 M - k(63.5 min)

Simplifying the equation, we get:

k = (0.970 M - 0.209 M) / 63.5 min

k = 0.761 M / 63.5 min

k = 0.01199 M/min, or approximately 0.012 M/min.

Answer 2

The value of k for the zero-order reaction a → products is approximately 0.01222 M/minute.

Step-by-step explanation:

In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactant. The integrated rate law for a zero-order reaction is given by the equation [A] = [A]o - kt, where [A] represents the concentration of the reactant at a given time, [A]o is the initial concentration of the reactant, k is the rate constant, and t is the time. To find the value of k for this reaction, we can use the given data:

[A]o = 0.970 M

[A] = 0.209 M

t = 63.5 minutes

Substituting these values into the integrated rate law equation and solving for k:

k = ([A]o - [A]) / t

k = (0.970 M - 0.209 M) / 63.5 minutes

k ≈ 0.01222 M/minute

Therefore, the value of k for this zero-order reaction is approximately 0.01222 M/minute.