(B) For a first order reaction,the rate constant $k$ is given by: $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$ Given: $[A]_0 = 0.05 \ M$,$[A]_t = 0.

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(B) For a first order reaction,the rate constant $k$ is given by: $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$ Given: $[A]_0 = 0.05 \ M$,$[A]_t = 0.05 - 0.015 = 0.035 \ M$,and $t = 45 \ min$. Substituting the values: $k = \frac{2.303}{45} \log \frac{0.05}{0.035} = \frac{2.303}{45} \log (1.4286) \approx 0.02673 \ min^{-1}$. The half-life period is: $t_{1/2} = \frac{0.693}{k} = \frac{0.693}{0.02673} \approx 25.92 \ min$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Easy

For a first order reaction,the initial concentration of a reactant is $0.05 \ M$. After $45 \ minutes$,it is decreased by $0.015 \ M$. Calculate the half-life period $(t_{1/2})$ (in $min$)?

GUJCET 2011 All GUJCET

A
$87.42$
B
$25.90$
C
$78.72$
D
$77.20$

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Chemical Kinetics

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First Order reaction

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For a first order reaction,the initial concentration of a reactant is $0.05 \ M$. After $45 \ minutes$,it is decreased by $0.015 \ M$. Calculate the half-life period $(t_{1/2})$ (in $min$)?

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The thermal decomposition of a molecule follows a first-order reaction. The molecule decomposes $50\%$ in $120 \text{ minutes}$. How many minutes will it take for $90\%$ decomposition?

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