Order of a Reaction

For the following elementary reaction, determine its order of reaction and the dimensions of the rate constant:

$2\text{NO}\left(\text{g}\right)\to {\text{N}}_2\text{O}\left(\text{g}\right)+\frac{1}{2}{\text{O}}_2$

For a reaction, $\mathrm{A}+2\mathrm{B}\to \mathrm{C}$, the rate is given by $+\frac{\mathrm{d}\left[\mathrm{C}\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]\left[\mathrm{B}\right]$, hence, the order of the reaction is:

Order of a reaction is the sum of exponents of _____ in the rate equation.

Rate constant and rate of a reaction have the same units for reactions of _____ order.

What is the order for the following reactions?
${\mathrm{CHCl}}_3 \left(\mathrm{g}\right) +{\mathrm{Cl}}_2 \left(\mathrm{g}\right) \to {\mathrm{CCl}}_4 \left(\mathrm{g}\right) +\mathrm{HCl} \left(\mathrm{g}\right)$, rate$=\mathrm{K}\left[{\mathrm{CHCl}}_3\right] [{\mathrm{Cl}}_2{]}^{1/2}$

The rate law for the gas-phase reaction $2\mathrm{NO} \left(\mathrm{g}\right)+ {\mathrm{O}}_2 \left(\mathrm{g}\right) \to 2{\mathrm{NO}}_2 \left(\mathrm{g}\right)$ is rate $=\mathrm{K}[{\mathrm{NO}}_2{]}^2 [{\mathrm{O}}_2].$ What is the order of the reaction with respect to each of the reactants and what is the overall order of the reaction?

Explain the term order of a reaction with examples.

The following results have been obtained during the kinetic studies of the reaction:

$2\mathrm{A}+\mathrm{B} \to \mathrm{C}+\mathrm{D}$

Determine the rate law and the rate constant for the reaction.

In a reaction between $\mathrm{A}$ and $\mathrm{B}$, the initial rate of reaction $\left({\mathrm{r}}_{\mathrm{o}}\right)$ was measured for different initial concentration of $\mathrm{A}$ and $\mathrm{B}$ as given below:

What is the order of the reaction with respect to $\mathrm{A}$ and $\mathrm{B}$?

If the rate v/s $[\mathrm{A}{]}^2$ graph is a straight line, the reaction is of second order.

The order of a reaction can be determined with the help of its rate law expression.

What is the order of a reaction which has a rate expression $\mathrm{r}\mathrm{a}\mathrm{t}\mathrm{e}=\mathrm{k}{\left[\mathrm{A}\right]}^{3/2}\mathrm{ }{\left[\mathrm{B}\right]}^{-1}$

The rate of the reaction,

$3\mathrm{A}+2\mathrm{B}\mathrm{ }\to \mathrm{ }\mathrm{P}\mathrm{r}\mathrm{o}\mathrm{d}\mathrm{u}\mathrm{c}\mathrm{t}\mathrm{s}$

is given by the rate expression :

$\mathrm{R}\mathrm{a}\mathrm{t}\mathrm{e}=\mathrm{k}\left[\mathrm{A}\right]{\left[\mathrm{B}\right]}^2$

If $\mathrm{A}$ is taken in excess, the order of the reaction would be :

If a certain reaction is first order with respect to $\mathrm{A},$ second order with respect to $\mathrm{B}$ and zero order with respect to $\text{C}$ then what is the order of reaction?

When initial concentration is doubled, the time for half-reaction is also doubled, the order of this reaction is:

From the rate expression for the following reaction, determine its order of reaction and the dimensions of the rate constant.

${\text{H}}_2{\text{O}}_2\left(\text{aq}\right)+3{\text{I}}^{-}\left(\mathrm{aq}\right)+2{\text{H}}^{+}⟶2{\text{H}}_2\text{O}\left(\mathrm{l}\right)+{\text{I}}_3^{-}\text{;}\text{Rate}=\mathrm{k}\left[{\text{H}}_2{\text{O}}_2\right]\left[{\text{I}}^{-}\right]$

For the following elementary reaction, determine its order of reaction and the dimensions of the rate constant:

$2\text{NO}\left(\text{g}\right)\to {\text{N}}_2\text{O}\left(\text{g}\right)+\frac{1}{2}{\text{O}}_2$

The rate law for reaction between the substances A and B is given by:

$\text{Rate}=\text{k}{\left[\text{A}\right]}^{\text{n}}{\left[\text{B}\right]}^{\text{m}}$

On doubling the concentration of A and halving the concentration of B, the ratio of the new rate to the earlier rate of reaction will be:

A reaction involving two different reactants can never be: