Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: AP EAPCET - 3 Sep 2021 Afternoon

Which one of the following statements is not correct?

For a reaction, the initial rate is given as ${\mathrm{R}}_0=\mathrm{k}{\left[{\mathrm{A}}_0\right]}^2\left[{\mathrm{B}}_0\right].$ By what factor, the initial rate of reaction will increase if the concentration of $\mathrm{A}$ taken is increased to $1.5$ times the original, and that of $\mathrm{B}$ is tripled?

For a certain reaction between $\mathrm{X}$ and $\mathrm{Y},$ the order with respect to $\mathrm{X}$ is $3$ and that with respect to $\mathrm{Y}$ is $4.$ If the concentrations of both $\mathrm{X}$ and $\mathrm{Y}$ are tripled. the rate of reaction will increase by a factor of ________

For the reaction $2\mathrm{A}+{\mathrm{B}}_2⟶2\mathrm{C},$ the following data is provided. Find the overall order of this reaction.

The half-life period of a first order reactor is $60$ minutes. If initial amount of the reactant taken is $50 \mathrm{g},$ the amount left after $4$ hrs. will be

Which expression among the following is correct for a zero-order reaction and a first order reaction respectively? Here $\text{'}a\text{'}$ denotes the intial concentration of reactant:

If the first order rate constants for the decomposition of ethyl iodide at $600 \mathrm{K}$ and $700 \mathrm{K}$ are $2.0\times {10}^{-5} {\mathrm{s}}^{-1}$ and $2.0\times {10}^{-4} {\mathrm{s}}^{-1}$ respectively, the activation energy for this reaction in ${\mathrm{kJmol}}^{-1}$ is