In a first-order reaction, the concentration of the reactant is reduced to one-fourth of its initial value in $50$ seconds. Calculate the rate constant of the reaction.

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Solution

$A = \frac{1}{4} A o$

$t = 50 s e c$

$K = ?$

$K = \frac{2.303}{50} \times l o g (4)$

$K = 0.027 {s e c}^{- 1}$

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In a first-order reaction, the concentration of the reactant is reduced to one-fourth of its initial value in 50 seconds. Calculate the rate constant of the reaction.

A=14Aot=50secK=?K=2.30350×log(4)K=0.027sec−1

In a first-order reaction, the concentration of the reactant is reduced to one-fourth of its initial value in $50$ seconds. Calculate the rate constant of the reaction.

$A = \frac{1}{4} A o$

$t = 50 s e c$

$K = ?$

$K = \frac{2.303}{50} \times l o g (4)$

$K = 0.027 {s e c}^{- 1}$