Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: Exercise 1

A catalyst increases the rate of reaction by:

In the Lindemann theory of unimolecular reactions, it is shown that the apparent rate constant for such a reaction is, ${\mathrm{k}}_{\mathrm{app} }=\frac{{\mathrm{k}}_1\mathrm{C}}{1+\mathrm{\alpha C}}$, where $\mathrm{C}$ is the concentration of the reactant ${\mathrm{k}}_1$ and $\mathrm{\alpha }$ is a constant. Calculate the value of $\mathrm{C}$ for which ${\mathrm{k}}_{\mathrm{app} }$ has $90\%$ of its limiting value, at $\mathrm{C}$ tending to infinitely large values. Given, $\mathrm{\alpha }=9\times {10}^5$.

Thermal decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ occurs as per the equation below: 

$2 {\mathrm{N}}_2{\mathrm{O}}_5\to 4{\mathrm{NO}}_2+{\mathrm{O}}_2$.

The correct statement is:

For an elementary reaction of reversible nature, net rate is: $\left(\frac{\mathrm{dx}}{\mathrm{dt}}\right)={\mathrm{k}}_1{\left[\mathrm{A}\right]}^2{\left[\mathrm{B}\right]}^1-{\mathrm{k}}_2\left[\mathrm{C}\right]$, hence, given reaction is:

The decay profiles of three radioactive species $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ are given below:

These profiles imply that the decay constants ${\mathrm{k}}_{\mathrm{A}}, {\mathrm{k}}_{\mathrm{B}}$ and ${\mathrm{k}}_{\mathrm{C}}$ follow the order:

Consider the following reversible first-order reaction of $\mathrm{X}$ at an initial concentration ${\left[\mathrm{X}\right]}_0$. The values of the rate constants are ${\mathrm{k}}_{\mathrm{f}}=2{\mathrm{s}}^{-1}$ and ${\mathrm{k}}_{\mathrm{b}}=1{\mathrm{s}}^{-1}$.

A plot of concentration of $\mathrm{X}$ and $\mathrm{Y}$ as function of time is:

Consider the reaction : $2{\mathrm{NO}}_2\left(\mathrm{g}\right)\to 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$. In the figure below, identify the curves $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ associated with the three species in the reaction.

For an elementary reaction, the net rate is $\left(\frac{\mathrm{dx}}{\mathrm{dt}}\right)=\mathrm{k}{\left[\mathrm{A}\right]}^2-{\mathrm{k}}^{\text{'}}\left[\mathrm{C}\right]{\left[\mathrm{B}\right]}^2$. Thus, select the correct statement: