Level 1

Thermal decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ occurs as per the equation below: 

$2 {\mathrm{N}}_2{\mathrm{O}}_5\to 4{\mathrm{NO}}_2+{\mathrm{O}}_2$.

The correct statement is:

For a $1^{\text{st }}$ order chemical reaction:

For a zero-order reaction with rate constant $\mathrm{k}$, the slope of the plot of reactant concentration against time is:

The rate constant of a chemical reaction at a very high temperature will approach:

A zero-order reaction, $\mathrm{A}\to$ Product, with an initial concentration ${\left[\mathrm{A}\right]}_0$ has a half-life of $0.2 \mathrm{s}$. If one starts with the concentration $2{\left[\mathrm{A}\right]}_0$, then the half-life is :

Among the following graphs showing variation of rate $\left(\mathrm{k}\right)$ with temperature $\left(\mathrm{T}\right)$ for a reaction, the one that exhibits Arrhenius behavior over the entire temperature range is:

The units of the rate constant of a first order reaction when time is measured in seconds is:

In a multi-step reaction, rate of the overall reaction is governed by the;