Odisha Board Solutions for Chapter: Chemical Kinetics, Exercise 1: QUESTIONS

The rate law for the reaction

$2\mathrm{A}+\mathrm{B}\to 2\mathrm{C}$  is represented as,

Rate $=\mathrm{k}{\left[\mathrm{A}\right]}^2 \left[\mathrm{B}\right]$. If A is taken in large excess, the order of the reaction will be,

If the rate of reaction between $\mathrm{A}$ and $\mathrm{B}$ is given by, rate $=\left[\mathrm{A}\right] {\left[\mathrm{B}\right]}^2$, then the reaction is,

The rate at which a substance reacts is proportional to:

Rate Expression of a chemical change is $\frac{\mathrm{dx}}{\mathrm{dt}}=\mathrm{k}{\left[\mathrm{A}\right]}^2 \left[\mathrm{B}\right] {\left[\mathrm{C}\right]}^0$

The order of the reaction is

A zero order reaction is one

The half-life period of a reaction is $100$ minutes. In $400$ minutes the initial concentration of $2.0 \mathrm{g}$ will become.

Which of the following rate law applies to a second order reaction involving only one reactant ?

In a second order reaction $2\mathrm{A}\to$products, the concentration is halved. The half life of the reaction is,