Chemistry · JEE

Elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units Mock Test for JEE

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Part of Chemical Kinetics in JEE Main Chemistry.

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Q1ChemistryUnit 8: Chemical Kinetics

A reaction

A+B \rightarrow C

is second order with respect to

A

and independent of

B

The rate expression for the reaction is:

Q2ChemistryUnit 8: Chemical Kinetics

Statement - I : The molecularity of the reaction

\boldsymbol{H}_{2}+\boldsymbol{B} \boldsymbol{r}_{2} \rightarrow 2 \mathrm{HBr}

is 2 Statement - II: The order of this reaction is

3 / 2

Q3ChemistryUnit 8: Chemical Kinetics

The choices below are some of the proposed steps of a reaction mechanism. Which step is least likely to be the ratedetermining step of the mechanism?

Q4ChemistryUnit 8: Chemical Kinetics

Which one of the following statements for order of reaction is not correct?

Q5ChemistryUnit 8: Chemical Kinetics

In the hydrolysis of organic chloride in the presence of a large excess of water,

\boldsymbol{R C l}+\boldsymbol{H}_{2} \boldsymbol{O} \rightarrow \boldsymbol{R O H}+\boldsymbol{H} \boldsymbol{C l}

Q6ChemistryUnit 8: Chemical Kinetics

For the reaction given below,

\mathbf{2} \mathbf{O}_{\mathbf{3}}(\mathbf{g}) \rightarrow \mathbf{3} \mathbf{O}_{\mathbf{2}}(\mathbf{g})

\operatorname{Step} \mid: \mathbf{O}_{3}(\mathbf{g}) \rightarrow \mathbf{O}_{2}(\mathbf{g})+\mathbf{O}(\mathbf{g})

Step

2: \mathrm{O}_{3}(\mathrm{g})+\mathrm{O} \rightarrow^{\text {slow }} 2 \mathrm{O}_{2}(\mathrm{g})

Statement I: The molecularity of the first step is 1 and of the second step is 2 Statement-II:

O(g)

is an intermediate and rate of reaction is

\mathbf{K}\left[\mathbf{O}_{3}\right]^{2}\left[\mathbf{O}_{2}\right]^{-1}

and order of reaction is 1

Q7ChemistryUnit 8: Chemical Kinetics

Which of the following statement is true for the reaction,

\boldsymbol{H}_{2}+\boldsymbol{B} \boldsymbol{r}_{2} \rightarrow \boldsymbol{2} \boldsymbol{H} \boldsymbol{B} \boldsymbol{r}

The rate law is

\frac{\boldsymbol{d} \boldsymbol{x}}{\boldsymbol{d} \boldsymbol{t}}=\boldsymbol{k}\left[\boldsymbol{H}_{2}\right]\left[\boldsymbol{B} \boldsymbol{r}_{2}\right]^{1 / 2}

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