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.

Order of a reaction with rate constant ${\text{mol}}^{-1}{\mathrm{L}}^{}{\mathrm{s}}^{-1}$ is :

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 $\mathrm{B}$?

Which one of the following statement for the order of the reaction is/are correct?

Suppose in a chemical reaction $\mathrm{A}\to \mathrm{B}$, it is found that the rate of the reaction doubles when the concentration of $\mathrm{A}$ is increased four times. The order of the reaction with respect to $\mathrm{A}$ is

In a given reaction condition N₂O₅ decomposes as

i) ${\text{N}}_2{\text{O}}_{5\left(\text{g}\right)}\rightleftharpoons {\text{N}}_2\text{O}\left(\text{g}\right)+2{\text{O}}_{2\left(\text{g}\right)}\text{; }{\text{K}}_{\text{c}}=2{\text{ M}}^2$

and same product competes to form N₂O₃

ii) ${\text{N}}_2\text{O}+{\text{O}}_2\rightleftharpoons {\text{N}}_2{\text{O}}_3$

If initially 1 mole of N₂O₅ was introduced into a one litre flask subjected to reaction conditions molar concentration of N₂O at equilibrium was found to be 0.2 M. Determine K_c for second reaction.

Concentration of reactant w.r.t. time varies as

The order of reaction is:

For a reaction $\mathrm{X}+\mathrm{Y}\to \mathrm{Z}$ , rate $\propto \left[\mathrm{X}\right]$ . What is (i) molecularity and (ii) order of reaction ?

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

For the reaction, $2A+B\to$ products, when the concentrations of $A$ and $B$ both were doubled, the rate of the reaction increased from $0.3mol{L}^{-1}$ to $2.4mol{L}^{-1}{s}^{-1}$. When the concentration of $A$ alone is doubled, the rate increased from $0.3mol{L}^{-1}{s}^{-1}$ to $0.6mol{L}^{-1}{s}^{-1}$.
Which one of the following statements is correct?

For the reaction, $2S{O}_2+O_2\left(\mathrm{e}\mathrm{x}\mathrm{c}\mathrm{e}\mathrm{s}\mathrm{s}\right)\to 2S{O}_3$ the order of reaction with respect to $O_2$ is

A hypothetical reaction,

$X_2+Y_2\to 2 XY$ follows the following mechanism

$X_2\rightleftharpoons X+X$ ........fast

$X+Y_2\to XY+Y$ ......slow

$X+Y\to XY$ .......fast

The order of the overall reaction is

For a chemical reaction $\mathrm{X}\mathrm{ }⟶\mathrm{ }\mathrm{Y},$ the rate of reaction increases by a factor 1.837 when the concentration of X is increased by 1.5 times. The order of the reaction with respect to X is