Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: TS EAMCET 2020 (9-Sep Shift-1)

The following results have been obtained during the kinetic studies of reaction:
$2\mathrm{NO}+2{\mathrm{H}}_2⟶{\mathrm{N}}_2+2{\mathrm{H}}_2\mathrm{O}$

What will be the overall order of a reaction for which the rate expression is given as
Rate$=\mathrm{K}\left[\mathrm{A}{]}^{\frac{1}{2}}\right[ \mathrm{B}{]}^{\frac{3}{2}}$

In the sequence of reaction $\mathrm{A}\stackrel{{\mathrm{k}}_1}{⟶}\mathrm{X}\stackrel{{\mathrm{k}}_2}{⟶}\mathrm{Y}\stackrel{{\mathrm{k}}_3}{⟶}\mathrm{Z}$ ${\mathrm{k}}_3>{\mathrm{k}}_2>{\mathrm{k}}_1,$ then the rate determining step is

For a first order reaction ${\mathrm{t}}_{1/2}$ is $1200 \mathrm{s}.$ The specific rate constant in ${\mathrm{s}}^{-1}$ is

The rate of chemical reaction doubles with every ${10}^o\mathrm{C}$ rise in temperature. If the reaction is carried out in the vicinity of ${22}^o\mathrm{C}$, the activation energy of the reaction is (Given $\mathrm{R}=8.3 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}, \ln 2=0.69$ and $\ln 3=1.1$)

If the rate constants of a reaction at $500 \mathrm{K}$ and $700 \mathrm{K}$ are $0.002 {\mathrm{s}}^{-1}$ and $0.06 {\mathrm{s}}^{-1}$, respectively, the value of activation energy is

$\left(\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}, \log 3=0.477\right)$

Calculate the activation energy of a reaction, whose rate constant doubles on raising the temperature from $300 \mathrm{K}$ to $600 \mathrm{K}.$