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**Problem**: The half-life of cesium-130 is 15 minutes. What percentage of the initial activity will be present after 75 minutes, assuming radioactive decay occurs by a first order rate mechanism?a. 0.312%b. 70.71%c. 4.25%d. 1.14%e. 3.13%

###### FREE Expert Solution

We’re being asked to determine the percentage of the initial activity of cesium-130 will be present after 75 minutes, assuming radioactive decay occurs by a first-order rate mechanism.

Recall that ** radioactive/nuclear decay of isotopes** follows first-order kinetics, and the integrated rate law for first-order reactions is:

$\overline{){\mathbf{ln}}{\mathbf{}}{\mathbf{\left[}\mathbf{N}\mathbf{\right]}}_{{\mathbf{t}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{kt}}{\mathbf{+}}{\mathbf{ln}}{\mathbf{}}{\mathbf{\left[}\mathbf{N}\mathbf{\right]}}_{{\mathbf{0}}}}$

where:

**[N] _{t}** = concentration at time t

**k** = decay constant

**t** = time

**[N] _{0}** = initial concentration.

Also, recall that ** half-life** is the time needed for the amount of a reactant to decrease by 50% or one-half.

The half-life of a first-order reaction is given by:

$\overline{){{\mathbf{t}}}_{\raisebox{1ex}{$\mathbf{1}$}\!\left/ \!\raisebox{-1ex}{$\mathbf{2}$}\right.}{\mathbf{=}}\frac{\mathbf{ln}\mathbf{}\mathbf{2}}{\mathbf{k}}}$

###### Problem Details

The half-life of cesium-130 is 15 minutes. What percentage of the initial activity will be present after 75 minutes, assuming radioactive decay occurs by a first order rate mechanism?

a. 0.312%

b. 70.71%

c. 4.25%

d. 1.14%

e. 3.13%

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