For a first order reaction A arrow Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min -1 is

Question

For a first order reaction A arrow Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min -1 is (A) 0.2303 (B) 1.3818 (C) 0.9212 (D) 0.4606

Tardigrade Admin · Accepted Answer

A arrow Products Initial conc. A o =0.1 M Conc. After 5 min At=0.001 M t =5 min. For first order reaction K =(2.303/ t ) log (( A o / A t )) =(2.303/5) log ((0.1/0.001)) K =0.9212 min -1

Q. For a first order reaction $A \to$ Products, initial concentration of $A$ is $0.1 M$ , which becomes $0.001 M$ after $5$ minutes. Rate constant for the reaction in $min^{- 1}$ is

$0.2303$

$1.3818$

$0.9212$

$0.4606$

A $\to$ Products
Initial conc. $A_{o} = 0.1 M$
Conc. After $5 min A_{t} = 0.001 M$
$t = 5 min$ .
For first order reaction
$K = \frac{2.303}{t} lo g (\frac{A _{o}}{A _{t}})$
$= \frac{2.303}{5} lo g (\frac{0.1}{0.001})$
$K = 0.9212 min^{- 1}$

Q. For a first order reaction A→ Products, initial concentration of A is 0.1M, which becomes 0.001M after 5 minutes. Rate constant for the reaction in min−1 is

0.2303

1.3818

0.9212

0.4606