Chemical kinetics practice · Medium

Assertion (A):The acid hydrolysis of ester takes place more rapidly in $\mathrm{D}_2 \mathrm{O}$ than $\mathrm{H}_2 \mathrm{O}$

Reason (R): $\mathrm{D}_3 \mathrm{O}^{+}$ is stronger acid than $\mathrm{H}_3 \mathrm{O}^{+}$ or $\mathrm{H}_2 \mathrm{D}^{+} \mathrm{O}$

A kinetic study of the reaction $\mathrm{A} \rightarrow \text{products}$ provides the data $t=0 \mathrm{~s},[\mathrm{A}]=2.00 \mathrm{~M} ;$ $500 \mathrm{~s},$ $1.00 \text{ M};$ $1500 \mathrm{~s},$ $0.50 \mathrm{M} ;$ $3500 \mathrm{~s},$ $0.25 \mathrm{~M}.$ In the simplest possible way determine whether this reaction is of

Assertion: Two different reaction can never have same rate of reaction

Reason: Rate of reaction always depends only on frequency of collision and Arrhenius factor

We are given with following information about concentration of reactant with initial rate of reaction.

$\begin{array}{cccccccccccccccccccc} {{\text{Initial concentration}}}&{{\text{Initial rate}}} \\ {0.005{\text{ M}}}&{7.5 \times {{10}^{ - 4}}} \\ {0.02{\text{ M}}}&{3 \times {{10}^{ - 3}}} \end{array}$

Find out order of reaction with respect to that reactant.

$\mathrm{T}_{50}$ of a first order reaction is $10 \mathrm{~min}$. Starting with $10 \mathrm{~mol} \mathrm{~L}^{-1}$, rate after $20 \mathrm{~min}$ is

Select the incorrect statement among the following

For the reaction $A \to B,$ the rate expression is $r = k{\left[ A \right]^n}.$ When the concentration of $A$ is doubled, the rate of reaction is quadrupled. The value of $n$ is

What is the role of a catalyst in a catalysed
reaction?

The rate of first order reaction are $0.8 \mathrm{~M} \mathrm{~min}^{-1}$ and $0.08\mathrm{~M} \mathrm{~min}^{-1}$ at 40 min and 60 min respectively. Then half life is:

The rate constant $\left( {k'} \right)$ of one of the reaction is found to be double that of the rate constant $\left( {k''} \right)$ of another reaction. Then the relationship between the corresponding activation energies of the two reaction $\left( {{{E'}_a}\;\mathrm{and}\;{{E''}_a}} \right)$ can be represented as

STATEMENT-1 : If the activation energy of reaction is zero, temperature will have no effect on the rate constant.

STATEMENT-2 : Lower the activation energy fasten is the reaction.

If the rate constant of the reaction, $X \rightarrow Y$ is $2.5 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ and initial concentration of $X$ is $3 \mathrm{~M}$ then the concentration of ${Y}$ after 100 minutes will be

After $20 \%$ completion, the rate of reaction $\mathrm{A} \rightarrow \text{products}$ is 10 unit and after $80 \%$ completion, the rate is 0.625 unit. The order of the reaction is

Statement I: Rate constants determined from Arrhenius equation are fairly accurate for simple as well as complex molecules

Statement II: Reactant molecules undergo chemical change irrespective of their orientation during collision

Following reaction takes places by mechanism

$\mathrm{NO}_2+\mathrm{CO} \longrightarrow \mathrm{NO}+\mathrm{CO}_2$
Step I $\mathrm{NO}_2+\mathrm{NO}_2 \xrightarrow{k_1 \text {. Slow }} \mathrm{NO}_3+\mathrm{NO}$

Step II $\mathrm{NO}_3+\mathrm{CO} \xrightarrow{k_2 \text {. Fast }} \mathrm{NO}_2+\mathrm{CO}_2$

Hence, $\left(\frac{d x}{d t}\right)$ for the given reaction is

The half-life for decay of radioactive ${ }^{14} {C}$ is 5730 years. An archaeological artefact containing wood has only $80 \%$ of the ${ }^{14} {C}$ activity as found in living trees. The age of the artefact would be [Given : $\log 1.25=0.0969$]

For a reaction of the type $A + B \to x$ products, it is observed that doubling the concentration of $A$ causes the reaction rate $({k_1})$ to be four times as great but doubling the amount of $B$ does not affect the rate $({k_2})$. The rate equation is

The inversion of cane sugar into glucose and fructose according to the equation ${\mathrm{C}_{12}}{\mathrm{H}_{22}}{\mathrm{O}_{11}} + {\mathrm{H}_2}\mathrm{O} \to {\mathrm{C}_6}{\mathrm{H}_{12}}{\mathrm{O}_6} + {\mathrm{C}_6}{\mathrm{H}_{12}}{\mathrm{O}_6}$ is an example of

The half-life period of a first order reaction is 1 min 40 s. Calculate its rate constant.

Rate of a reaction $\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}$ is given below as a function of differential concentrations of $\mathrm{A}$ and $\mathrm{B}$.

$\begin{array}{cccccccccccccccccccc} {{\text{Exp}}{\text{.}}}&{\left[ {\text{A}} \right]}&{\left[ {\text{B}} \right]}&{{\text{Rate}}} \\ {}&{{\text{mol }}{{\text{L}}^{ - 1}}}&{{\text{mol }}{{\text{L}}^{ - 1}}}&{{\text{mol }}{{\text{L}}^{ - 1}}\,{\text{tim}}{{\text{e}}^{ - 1}}} \\ {1.}&{0.01}&{0.01}&{0.005} \\ {2.}&{0.02}&{0.01}&{0.010} \\ {3.}&{0.01}&{0.02}&{0.005} \end{array}$

Determine the order of reaction with respect to $\mathrm{A}$ and and also calculate the half-life of $\mathrm{A}$ in the reaction.

Rate constant $(\mathrm{K})$ varies with temperature as given by equation $\log \mathrm{K}\left(\mathrm{min}^{-1}\right)=5-\frac{2000}{\mathrm{T}}$
Consider the following about this equation
(I) Pre exponential factor is $10^5$.
(II) $\mathrm{E}_\alpha$ is $9.212 \mathrm{~kcal}$.
(III) Variation of $\log \mathrm{K}$ with $1 / \mathrm{T}$ is linear.
Select the correct statement.

If the initial concentration of reactants are doubled half life becomes half. Then order of the reaction will be

For the elementary reaction $2 \mathrm{NO}+\mathrm{O}_2 \rightarrow 2 \mathrm{NO}_2,$ the volume of a container is tripled. The rate becomes

The rate for the reaction, $RCl + NaOH\left( {aq} \right) \to ROH + NaCl$ is given by $rate\mathrm{ } = K_1\left[ {RCl} \right].$ The rate of the reaction is

When two reactants $A$ and $B$ are mixed to give products $C$ and $D$, the reaction quotient $Q$ at the initial stage of the reaction is best described by-

Assertion: Hydrolysis of methyl ethanoate is a pseudo first order reaction.

Reason: Water is present in large excess and therefore its concentration remained constant throughout the reaction.

If half life of radioactive bromine ( $\mathrm{Br}-82)$ is $36 \mathrm{hr}$, find percentage remaining after one day. [nearest integer]

What is not correct for a zero order reaction

A first order reaction has a specific reaction rate of $10^{-1} \mathrm{~s}^{-1}$. How much time will it take for $100 \mathrm{~g}$ of its reactant to be reduced to $25 \mathrm{~g}$?

For the reaction,

${\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{B}{\mathrm{r}_2}\left( \mathrm{g} \right) \to 2\mathrm{HBr}\left( \mathrm{g} \right)$

The experimental data suggest

$\mathrm{rate} = k\left[ {{\mathrm{H}_2}} \right]{\left[ {\mathrm{B}{\mathrm{r}_2}} \right]^{1/2}}$

the molecularity and order of the reaction are respectively