(A) Step $1$: Calculate the concentration after $1 \ hour$ $(60 \ min)$.For a first-order reaction: $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$.$\l

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$3.4354 \times 10^{-3} \ M \ min^{-1}$

(A) Step $1$: Calculate the concentration after $1 \ hour$ $(60 \ min)$.For a first-order reaction: $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$.$\log \frac{[A]_0}{[A]_t} = \frac{kt}{2.303} = \frac{4.5 \times 10^{-3} \ min^{-1} \times 60 \ min}{2.303} = 0.11726$.$\frac{[A]_0}{[A]_t} = \text{antilog}(0.11726) = 1.310$.$[A]_t = \frac{1 \ M}{1.310} = 0.7633 \ M$.Step $2$: Calculate the rate after $60 \ min$.Rate $= k[A]_t = 4.5 \times 10^{-3} \ min^{-1} \times 0.7633 \ M = 3.435 \times 10^{-3} \ M \ min^{-1}$.

Class 12 Chemistry Chemical Kinetics First Order reaction

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For the first-order isomerization reaction $A \rightarrow B$,the rate constant is $4.5 \times 10^{-3} \ min^{-1}$. If the initial concentration of $A$ is $1 \ M$,find the rate of the reaction after $1 \ hour$.

A
$3.4354 \times 10^{-3} \ M \ min^{-1}$
B
$4.3354 \times 10^{-3} \ M \ min^{-1}$
C
$3.4354 \times 10^{-5} \ M \ min^{-1}$
D
$3.4354 \times 10^{-9} \ M \ min^{-1}$

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Chemical Kinetics

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First Order reaction

For the first-order gaseous reaction $A_{(g)} \to 2B_{(g)} + C_{(g)}$,the expression for the rate constant $K$ in terms of initial pressure $P_0$ and total pressure $P_t$ at time $t$ is:

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For a first order reaction,show that the time required for $99 \%$ completion is twice the time required for the completion of $90 \%$ of the reaction.

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Reaction $A_{(g)} \rightarrow 2B_{(g)} + C_{(g)}$ is a first order reaction. It was started with pure $A$.
$t/min$ Pressure of system at time $t/mm \ Hg$
$10$ $160$
$\infty$ $240$
Which of the following option is incorrect?

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Which equation represents the $1/4^{th}$ life for a first-order reaction?

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The decomposition of substance $A$ follows first-order kinetics. Flask $I$ contains $1 \ L$ of $1 \ M$ solution of $A$,and flask $II$ contains $100 \ mL$ of $0.6 \ M$ solution of $A$. After $8 \ hours$,the concentration of $A$ in flask $I$ becomes $0.25 \ M$. How many hours will it take for the concentration of $A$ in flask $II$ to become $0.3 \ M$?

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$t/min$	Pressure of system at time $t/mm \ Hg$
$10$	$160$
$\infty$	$240$

For the first-order isomerization reaction $A \rightarrow B$,the rate constant is $4.5 \times 10^{-3} \ min^{-1}$. If the initial concentration of $A$ is $1 \ M$,find the rate of the reaction after $1 \ hour$.

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For the first-order gaseous reaction $A_{(g)} \to 2B_{(g)} + C_{(g)}$,the expression for the rate constant $K$ in terms of initial pressure $P_0$ and total pressure $P_t$ at time $t$ is:

For a first order reaction,show that the time required for $99 \%$ completion is twice the time required for the completion of $90 \%$ of the reaction.

Reaction $A_{(g)} \rightarrow 2B_{(g)} + C_{(g)}$ is a first order reaction. It was started with pure $A$.$t/min$Pressure of system at time $t/mm \ Hg$$10$$160$$\infty$$240$Which of the following option is incorrect?

Which equation represents the $1/4^{th}$ life for a first-order reaction?

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Reaction $A_{(g)} \rightarrow 2B_{(g)} + C_{(g)}$ is a first order reaction. It was started with pure $A$.
$t/min$ Pressure of system at time $t/mm \ Hg$
$10$ $160$
$\infty$ $240$
Which of the following option is incorrect?