Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 2: EXERCISE-2

At certain temperature, the half life period in the thermal decomposition of a gaseous substance as follows:

Find the order of reaction [Given $\log (23.5)=1.37;\log \left(95\right)=1.97]$

The rate of a reaction gets doubled when the temperature changes from $7°\mathrm{C}$ to $17°\mathrm{C}$. By which factor will it change for the temperature change from $17°\mathrm{C}$ to $27°\mathrm{C}$ ?

For the reaction $\mathrm{A}+2 \mathrm{B}\to$ products (started with concentrations taken in stoichiometric proportion), the experimentally determined rate law is :

 $-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=\mathrm{k} \sqrt{\left[\mathrm{A}\right] }\sqrt{\left[\mathrm{B}\right]}$

The half life time of the reaction would be:

A first order reaction is $25\%$ completed in $20$ minutes at $300 \mathrm{K}$. When same reaction in carried out at $320 \mathrm{K}$, it is $25\%$ complete in 5 minute. What is the activation energy of reaction (in $\mathrm{kJ}/\mathrm{mole}$ )?

[Take : $\mathrm{R}=8 \mathrm{J}/\mathrm{K}$ mole and $\ln 2=0.7]$

For the reaction $\mathrm{A}\to \mathrm{B}$, the rate law expression is $-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=\mathrm{k}{\left[\mathrm{A}\right]}^{1/2}$. If initial concentration of $\left[\mathrm{A}\right]$ is ${\left[\mathrm{A}\right]}_0$, then :

For the first order decomposition of ${\mathrm{SO}}_2{\mathrm{Cl}}_2\left(\mathrm{g}\right)$,

$\left[{\mathrm{SO}}_2{\mathrm{Cl}}_2\left(\mathrm{g}\right)\to {\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\right]$

a graph of $\log \left({\mathrm{a}}_0-\mathrm{x}\right)$ vs $\mathrm{t}$ is shown in figure. What is the rate constant $\left({\sec }^{-1}\right)$ ?

Consider the reaction $\mathrm{A}⟶\mathrm{B}$, graph between half life $\left({\mathrm{t}}_{1/2}\right)$ and initial concentration (a) of the reactant is

Hence, graph between$-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}$ And time will be

Select incorrect statement (s):