The rate constant for an isomerization reaction: A ⟶B, is 4.5 ×10^-3 min^-1 . If the initial co

Name: Problem 124, Chapter 4: Objective Chemistry for NEET Vol II
Uploaded: 2022-02-12T19:25:57-08:00
Duration: 36 s
Channel: Mishal Gul
Description: The rate constant for an isomerization reaction: A ⟶B, is 4.5 ×10^-3 min^-1 . If the initial concen- tration of A is 1 M, calculate the rate of reaction after I hour: (a) 0.34354 Mmin^-1 (b) 0.034354 M min^-1 (c) 0.0034354 M min^-1 (d) 0.0003454 M min^-1

step 1 The rate constant for an isomerization reaction A forming B is 4 .5 into 10 raise to power minus

Question

The rate constant for an isomerization reaction: $\mathrm{A} \longrightarrow \mathrm{B}$, is $4.5 \times 10^{-3} \mathrm{~min}^{-1} .$ If the initial concen- tration of $\mathrm{A}$ is $1 \mathrm{M}$, calculate the rate of reaction after I hour: (a) $0.34354 \mathrm{Mmin}^{-1}$ (b) $0.034354 \mathrm{M} \mathrm{min}^{-1}$ (c) $0.0034354 \mathrm{M} \mathrm{min}^{-1}$ (d) $0.0003454 \mathrm{M} \mathrm{min}^{-1}$

   The rate constant for an isomerization reaction:
$\mathrm{A} \longrightarrow \mathrm{B}$, is $4.5 \times 10^{-3} \mathrm{~min}^{-1} .$ If the initial concen-
tration of $\mathrm{A}$ is $1 \mathrm{M}$, calculate the rate of reaction after I hour:
(a) $0.34354 \mathrm{Mmin}^{-1}$
(b) $0.034354 \mathrm{M} \mathrm{min}^{-1}$
(c) $0.0034354 \mathrm{M} \mathrm{min}^{-1}$
(d) $0.0003454 \mathrm{M} \mathrm{min}^{-1}$

Objective Chemistry for NEET Vol II

Pearson Education 2nd Edition

Chapter 4, Problem 124

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Solved by Expert Mishal Gul

02/12/2022

Step 1

Step 1: The rate of reaction for a first order reaction is given by the equation: \[Rate = k[A]\] where $k$ is the rate constant and \([A]\] is the concentration of reactant A. Show more…

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The rate constant for an isomerization reaction: $\mathrm{A} \longrightarrow \mathrm{B}$, is $4.5 \times 10^{-3} \mathrm{~min}^{-1} .$ If the initial concen- tration of $\mathrm{A}$ is $1 \mathrm{M}$, calculate the rate of reaction after I hour: (a) $0.34354 \mathrm{Mmin}^{-1}$ (b) $0.034354 \mathrm{M} \mathrm{min}^{-1}$ (c) $0.0034354 \mathrm{M} \mathrm{min}^{-1}$ (d) $0.0003454 \mathrm{M} \mathrm{min}^{-1}$

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Key Concepts

First-Order Reaction Kinetics

In first-order reactions, the reaction rate depends linearly on the concentration of a single reactant. This means that as the concentration decreases, the reaction rate also decreases proportionally over time, which is particularly useful for describing processes such as isomerization reactions.

Integrated Rate Law

The integrated rate law for a first-order reaction, given by [A] = [A]? exp(?kt), relates the concentration of the reactant at any time to its initial concentration and the rate constant. This equation is crucial for calculating the remaining concentration after a given period of time.

Rate Constant

The rate constant (k) is a parameter that quantifies the speed of the reaction. In the context of first-order kinetics, it appears in both the differential rate law, where the rate is proportional to [A], and the integrated rate law, determining the rate of the exponential decay of the reactant concentration.

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