Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 2: EXERCISE-I (Conceptual Questions)

The specific rate constant of a first order reaction depends upon the,

The rate law of the reaction, $\mathrm{A}+2\mathrm{B}\to$ Product, is given by $\frac{\mathrm{d}\left(\text{product}\right)}{\mathrm{dt}}=\mathrm{k}{\left[\mathrm{A}\right]}^2\left[\mathrm{B}\right].$ If $\mathrm{A}$ is taken in excess, the order of the reaction will be:

The reaction $2\mathrm{A}+\mathrm{B}\to$product; follows the mechanism:
$2\mathrm{A}\rightleftharpoons {\mathrm{A}}_2$ (fast)
${\mathrm{A}}_2+\mathrm{B}\to \mathrm{P}$ (slow)
The order of the reaction is:

$\mathrm{k}$ for a zero order reaction is $2\times {10}^{-2} \mathrm{mol} {\mathrm{L}}^{-1} {\mathrm{s}}^{-1}$. If the concentration of the reactant after $25 \mathrm{s}$ is $0.5 \mathrm{M},$ the initial concentration must have been

In a first order reaction the $\mathrm{a}/(\mathrm{a}-\mathrm{x})$ was found to be $8$ after $10$ minute. The rate constant $\left({\min }^{-1}\right)$ is:

$75\%$ of a first order reaction was completed in $32 \min .$ When was $50\%$ of the reaction completed?

The half life for the reaction ${\mathrm{N}}_2{\mathrm{O}}_5\rightleftharpoons 2{\mathrm{NO}}_2+\frac{1}{2}{\mathrm{O}}_2$ is $24 \mathrm{hrs}$ at $30°\mathrm{C}$. Starting with $10 \mathrm{g}$ of ${\mathrm{N}}_2{\mathrm{O}}_5$ how many grams of ${\mathrm{N}}_2{\mathrm{O}}_5$ will remain after a period of $96$ hours:

At room temperature, the reaction between $\mathrm{NO}$ and ${\mathrm{O}}_2$ to give ${\mathrm{NO}}_2$ is fast, while that between $\mathrm{CO}$ and ${\mathrm{O}}_2$ is slow. It is due to: