Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 5: Exercise-5

For a gaseous reaction $\mathrm{A}\to$products, the half-life of the first order decomposition at $400 \mathrm{K}$ is $150$ minutes and the energy of activation is $65.0 \mathrm{kJ} {\mathrm{mole}}^{-1}.$ What fraction of molecules of $\mathrm{A}$ at $400 \mathrm{K}$ have sufficient energy to give the products?

At some temperature, the rate constant for the decomposition of $\mathrm{HI}$ on a gold surface is $0.1 {\mathrm{Ms}}^{-1}.$

$2\mathrm{HI}\to {\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$

What is the order of the reaction? How long will it take for the concentration of $\mathrm{HI}$ to drop from $2 \mathrm{M} \mathrm{to} 0.5 \mathrm{M}$.

A certain reaction $\mathrm{A}+\mathrm{B}\to \mathrm{C},$ the first order with respect to each reactant $\mathrm{k}={10}^{-3}.$ Determine the final concentration of $\mathrm{A}$ after $100 \mathrm{s},$ if the initial concentration of $\mathrm{A}$ was $0.1 \mathrm{M}$ and that of $\mathrm{B}$ was $0.2 \mathrm{M}.$

For the complex, ${\mathrm{Ag}}^{+}+2{\mathrm{NH}}_3\rightleftharpoons \left[\mathrm{Ag}\left({\mathrm{NH}}_3\right){}_2^{+}\right]$

$\left(\frac{\mathrm{dx}}{\mathrm{dt}}\right)=2\times {10}^7{\mathrm{L}}^2{\mathrm{mol}}^{-2}{\mathrm{s}}^{-1}\left[{\mathrm{Ag}}^{+}\right]{\left[{\mathrm{NH}}_3\right]}^2-1\times {10}^{-2}{\mathrm{s}}^{-1} \left[\mathrm{Ag}{{\left({\mathrm{NH}}_3\right)}_2}^{+}\right]$

Hence, ratio of rate constants of the forward and backward reaction is:

Consider the elementary reaction sequence shown in figure. Which of the following equation correct?

$\mathrm{A}\left(\mathrm{aq}\right)\to \mathrm{B}\left(\mathrm{aq}\right)+\mathrm{C}\left(\mathrm{aq}\right)$ is a first order reaction,

Reaction progress is measure with the help of titration of reagent $\text{'}\mathrm{R}\text{'}.$ If all $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ reacted with reagent and have $\text{'}\mathrm{n}\text{'}$ factors [$\mathrm{n}$ factors; eq.wt $=\frac{\mathrm{mol}. \mathrm{wt}}{\mathrm{n}}$] in the ratio of $1:2:3$ with the reagent. The $\mathrm{k}$ in terms of $\mathrm{t}, {\mathrm{n}}_1 \mathrm{and} {\mathrm{n}}_2$ is:

For $\mathrm{A}\underset{{\mathrm{K}}_1}{\to }\mathrm{B}\underset{{\mathrm{K}}_2}{\to }\mathrm{C},$is characterised by:

Decomposition of ${\mathrm{H}}_2{\mathrm{O}}_2$ is a first-order reaction. A solution of ${\mathrm{H}}_2{\mathrm{O}}_2$ labeled as $20$ volumes was left open. Due to this, some ${\mathrm{H}}_2{\mathrm{O}}_2$ is decomposed. To determine the new volume strength after $6$ hours, $10 \mathrm{mL}$ this solution was diluted to $100 \mathrm{mL}. 10 \mathrm{mL}$ of this diluted solution was titrated against $25 \mathrm{mL}$ of $0.025 \mathrm{M} {\mathrm{KMnO}}_4$ solution under acidic conditions. Calculate the rate constant for the decomposition of ${\mathrm{H}}_2{\mathrm{O}}_2$ in ${\mathrm{second}}^{-1}.$ Report your answer as $\mathrm{K}\times {10}^6$. $\left[\ln \frac{20}{17.5}=0.1335\right]$