Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: TS EAMCET - 9 August 2021 Shift 2

For a first order reaction $(\mathrm{A}⟶\mathrm{P})$ the rate constant is $5\times {10}^{-3} {\min }^{-1}$ when the initial concentration of $\mathrm{A}=2\times {10}^{-2} \mathrm{M}$. If the initial concentration of $\mathrm{A}$ is doubled, what will be the rate constant (in ${\min }^{-1}$) at the same temperature?

For a chemical reaction $\mathrm{A}+\mathrm{B}\underset{{\mathrm{k}}_{-1}}{\overset{{\mathrm{k}}_1}{\rightleftarrows }}\mathrm{C}\stackrel{{\mathrm{k}}_2}{⟶}\mathrm{D}.$ The rate $\frac{\mathrm{dc}}{\mathrm{dt}}$ is,

For the reaction of the type $\mathrm{A}+\mathrm{B}\to$ products, it is observed that doubling the concentration of $\mathrm{A}$ increases the reaction rate by four times, but doubling the concentration of $\mathrm{B}$ there is no apparent effect on the rate. The rate equation is

${\mathrm{x}}_2\left(\mathrm{g}\right)+{\mathrm{y}}_2\left(\mathrm{g}\right)\to 2\mathrm{xy}\left(\mathrm{g}\right)$ the experimental data indicates that rate $=\mathrm{k}\left[{\mathrm{x}}_2\right]{\left[{\mathrm{y}}_2\right]}^{1/2}.$ The molecularity and the order of reaction, respectively, are

If a first order reaction is found to have a rate constant of $1.386\times {10}^{-12} {\mathrm{s}}^{-1}$, the half life of the reaction in $\mathrm{s}$ is ? [Report answer in $\mathrm{seconds}$]

If a catalyst drops the activation energy of a reaction at ${27}^o\mathrm{C}$ from $100 \mathrm{kJ}/\mathrm{mol}$ to $42.73 \mathrm{kJ}/\mathrm{mol}$. The magnitude of the effect on forward and backward reaction is

The rate constant of a reaction at $25°\mathrm{C}$ is $1\times {10}^{-3}{ \min }^{-1}.$ If the temperature coefficient of the reaction is $2,$ the rate constant $\left({\min }^{-1}\right)$ at $15°\mathrm{C}$ is