Question

The rate constant for a certain first order decomposition reaction is 0.23 s–1 at 673K. Calculate the half-change period for this reaction.

Answer 1

Answer : The half-change period for this reaction is 3.01 seconds.

Explanation :

Rate constant of the reaction = $0.23s^{-1}$

The formula used for first order reaction of half-life is:

$k=\frac{0.693}{t_{1/2}}$

where,

k = rate constant of the reaction

$t_{1/2}$ = half-life of the reaction

Now put all the given values in the above formula, we get:

$k=\frac{0.693}{t_{1/2}}$

$t_{1/2}=\frac{0.693}{k}$

$t_{1/2}=\frac{0.693}{0.23s^{-1}}$

$t_{1/2}=3.01s$

Therefore, the half-change period for this reaction is 3.01 seconds.