For the following zero-order reaction, the half-life is 46.5 seconds and the initial concentration \([A]_0 = 1.39 \, \text{M}\). Calculate the rate constant.

\[ 2A \rightarrow 3B \]

Express your answer in \(\text{M/s}\).

For a zero-order reaction, the rate constant (k) can be calculated using the formula: k = [A]0 / (2*t1/2). Given the values of the half-life (t1/2) as 46.5 and the initial concentration [A]0 as 1.39, the rate constant is calculated to be approximately 0.015 M/s.

Explanation:

The question is asking for the rate constant of a zero-order reaction. The half-life of such a reaction can be calculated using the formula t1/2 = [A]0/2k, where [A]0 is the initial concentration of the reactant, t1/2 is the half-life of the reaction, and k is the rate constant.

In this case, we have the half-life (t1/2) as 46.5, and the initial concentration [A]0 as 1.39. Plugging these values into our formula, we can then calculate the rate constant (k) as: k = [A]0 / (2*t1/2) or k = 1.39/(2*46.5), which gives us an answer of 0.015 M/s for the rate constant.

Learn more about Rate Constant here:

https://brainly.com/question/32987256

#SPJ11

For the following zero-order reaction, the half-life is 46.5 seconds and the initial concentration \([A]_0 = 1.39 \, \text{M}\). Calculate the rate constant.\[ 2A \rightarrow 3B \]Express your answer in \(\text{M/s}\).

Answer :

Final answer:

Explanation:

Learn more about Rate Constant here:

Other Questions

For the following zero-order reaction, the half-life is 46.5 seconds and the initial concentration \([A]_0 = 1.39 \, \text{M}\). Calculate the rate constant.

\[ 2A \rightarrow 3B \]

Express your answer in \(\text{M/s}\).