The rate constant (k) for a first-order reaction can be calculated using the formula:

k = 0.693 / t1/2

where t1/2 is the half-life of the reaction. In this case, the half-life (t1/2) of Radon (Rn) is 3.823 days.

So, substituting the given half-life into the formula, we get:

k = 0.693 / 3.823

After performing the division, we find that the rate constant (k) is approximately 0.181 days^-1.

Question

The rate constant (k) for a first-order reaction can be calculated using the formula:

k = 0.693 / t1/2

where t1/2 is the half-life of the reaction. In this case, the half-life (t1/2) of Radon (Rn) is 3.823 days.

So, substituting the given half-life into the formula, we get:

k = 0.693 / 3.823

After performing the division, we find that the rate constant (k) is approximately 0.181 days^-1.

Knowee AI · Accepted Answer

The rate constant (k) for a first-order reaction can be calculated using the formula:

k = 0.693 / t1/2

where t1/2 is the half-life of the reaction. In this case, the half-life (t1/2) of Radon (Rn) is 3.823 days.

So, substituting the given half-life into the formula, we get:

k = 0.693 / 3.823

After performing the division, we find that the rate constant (k) is approximately 0.181 days^-1.

Radon (Rn) decays in a first-order process with a half-life of 3.823 days. What is thevalue of the rate constant in days -1 ?