Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: BITSAT 2017

Given the hypothetical reaction mechanism

$\mathrm{A}\stackrel{\mathrm{I}}{⟶}\mathrm{B}\stackrel{\mathrm{II}}{⟶}\mathrm{C}\stackrel{\mathrm{III}}{⟶}\mathrm{D}\stackrel{\mathrm{IV}}{\to } \mathrm{E}$ and the rate as

The rate determining step is

For the chemical reaction

$2{\mathrm{O}}_3⟶3{\mathrm{O}}_2$, the reaction proceeds as follows

${\mathrm{O}}_3\rightleftharpoons {\mathrm{O}}_2+\mathrm{O}$ (Fast)

$\mathrm{O}+{\mathrm{O}}_3⟶2{\mathrm{O}}_2$, (Slow)

the rate law expression should be given as

For a reversible reaction, $\mathrm{A}\rightleftharpoons \mathrm{B}$, which one of the following statement is wrong from the given energy profile diagram?

Under the same reaction conditions, initial concentration of $1.386 \mathrm{mol} {\mathrm{dm}}^{-3}$ of a substance becomes half in $40 \mathrm{s}$ and $20 \mathrm{s}$ through first order and zero order kinetics, respectively. Ratio $\left(\frac{{\mathrm{k}}_1}{{\mathrm{k}}_0}\right)$ of the rate of constants for first order $\left({\mathrm{k}}_1\right)$ and zero order $\left({\mathrm{k}}_0\right)$ of the reaction is

The rate of a reaction triples when temperature changes from ${20}^0\mathrm{C}$ to ${50}^0\mathrm{C}$. The energy of activation for the reaction is $\left(\mathrm{R}=8.314{\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}\right)$

Which of the following expression is correct for the rate of reaction given below ?

$5{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)+{\mathrm{BrO}}_3^{-}\left(\mathrm{aq}\right)+6{\mathrm{H}}^{+}\left(\mathrm{aq}\right)⟶3{\mathrm{Br}}_2\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

For an endothermic reaction, where $\mathrm{\Delta H}$ represent the enthalpy of reaction in $\mathrm{kJ} {\mathrm{mol}}^{-1}$, the minimum value for energy of activation (for forward reaction) will be

A graph is plotted between log $\mathrm{K}$ versus $\frac{1}{\mathrm{T}}$ for calculation of activation energy $\left({\mathrm{E}}_{\mathrm{a}}\right)$. The correct plot is