Chemical kinetics practice · Mixed difficulty

For the reaction $\mathrm{X \longrightarrow Y+Z}$ the following were obtained.

$\begin{array}{cccccccccccccccccccc} {{\text{Time}}}&0&{900}&{1800} \\ {{\text{Conc}}{\text{. of X}}}&{50.7}&{19.6}&{7.61} \end{array}$

Find the order of the reaction.

For a reaction the initial rate is given as: $R_0=k[A]_0^2[B]_0$ by what factor, the initial rate of reaction will increase if initial concentration of $A$ is taken 1.5 times and of $B$ is tripled?

For a first order reaction $k = 100\;{\mathrm{s}^{ - 1}}\mathrm{.}$ The time for completion of 50% reaction is

The slope of Arrhenius plot $\left( {\ln \,k\,\mathrm{v/s}\frac{1}{T}} \right)$ of first order reaction is $- 5 \times {10^3}K.$ The value of ${E_a}$ of the reaction is.
Choose the correct option for your answer.
[Given $R = 8.314\mathrm{ J}{\mathrm{K}^{ - 1}}\mathrm{ mo}{\mathrm{l}^{ - 1}}$]

Assertion (A):Threshold energy of a reaction is dependent of temperature.

Reason (R):The energy of activation decreases with increase in temperature.

The rate of reaction increases with temperature due to

Consider the following statements.

a. For zero order reaction $t_{1 / 2}$ is directly proportional to the initial concentration of the reactants.

b. Inversion of cane sugar is an example of pseudo first order reaction.

c. Decomposition of gaseous ammonia on a hot platinum surface is a zero order reaction at high pressure.

The correct statement are

Half-life period of second order reaction is

A first order reaction is half-completed in $45 \mathrm{~min}$. How long does it need for $99.9 \%$ of the reaction to be completed?

Rate of reaction depends upon

Which of the following statements are correct?

1. Order of a reaction can be known from experimental result and not from the stoichiometry of reaction

2. Overall molecularity of a reaction may be determined in a manner similar to overall order of reaction

3. Overall order of reaction,

${A^m} + {B^n} \to A{B_x}\;is\;\left( {m + n} \right)$

4. Molecularity of a reaction refers to

(i) Molecularity of each of the elementary steps (slow steps) in a multistep reaction

(ii) Molecularity of that particular step in a single step reaction

Select the correct answer by using the codes given below

For a homogeneous gaseous reaction $\mathrm{A} \longrightarrow 3 \mathrm{B}$, if pressure after time $\mathrm{t}$ was $\mathrm{P}_{\mathrm{t}}$ and after completion of reaction, pressure was $\mathrm{P}_{\infty}$ then select correct relation

Which is correct relation in between $\frac{{dc}}{{dt}},\frac{{dn}}{{dt}}\;and\;\frac{{dP}}{{dt}},$ where $c,n\;and\;p$, represent concentration, mole and pressure terms for gaseous phase reactant $A\left( \mathrm{g} \right) \to products$?

For zero order reaction the integrated rate equation is

An increase in the concentration of reactants of a reaction leads to change in

For the two gaseous reactions, following data are given,

$A \to B;\;{k_1} = {10^{10}}\;{e^{ - 20,000/T}}$

$C \to D;\;{k_2} = {10^{12}}\;{e^{ - 24,606/T}}$

The temperature at which ${k_1}$ becomes equal to ${k_2}$ is

Statement-1: The reciprocal of time in which $66\%$ of the reactant is converted to product is equal to the rate constant of first order reaction.
Statement-2: The rate constant for first order reaction depends on initial concentration of reactants.

For the reaction, $2 \mathrm{NO}_2(g)+\mathrm{F}_2(g) \longrightarrow 2 \mathrm{NO}_2 \mathrm{~F}(g)$
Steps are

I. $\mathrm{NO}_2(g)+\mathrm{F}_2(g) \stackrel{k_1}{\underset{k_2}{\rightleftharpoons}} \mathrm{NO}_2 \mathrm{~F}_2(g)$ (Fast)

II. $\mathrm{NO}_2 \mathrm{~F}_2(g) \xrightarrow{k_3} \mathrm{NO}_2 \mathrm{~F}(g)+\mathrm{F}(g)$ (Slow)

III. $\mathrm{F}(g)+\mathrm{NO}_2(g) \xrightarrow{k_4} \mathrm{NO}_2 \mathrm{~F}(g)$ (Fast)

Select the correct statement(s).

Select the incorrect statement :

The rate constant for a reaction is $10.8 \times {10^{ - 5}}\,\,mol.{L^{ - 1}}.{S^{ - 1}}$ the reaction obeys

The ratio of the times for 99.9% of the reaction to complete and half of the reaction to complete is

The rate constant of the reaction $A \to B$ is $0.6 \times {10^{ - 3}}$ mole per second. If the concentration of A is 5M, then concentration of B after 20 minutes is:

Assertion : If the activation energy of a reaction is zero, temperature will have no effect on the rate constant.

Reason : Lower the activation energy, faster is the reaction.

In a reaction: $A \to B,$ the concentration of ‘$A$’ at time 10 s and 20 s is $2.2\,{\text{mol}}\,{{\text{L}}^{ - 1}}$ and $1.1\,{\text{mol}}\,{{\text{L}}^{ - 1}}.$
The average rate of the reaction during the time period is

Correct statements in the following are

a) In $\mathrm{Hg}_{(t)}+\mathrm{Cl}_{2(g)} \rightarrow \mathrm{HgCl}_{2(s)}$, the rate of disappearance of any of the reactants is same as the rate of appearance of the product

b) In $2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}$, the rate of consumption of $\mathrm{HI}$ is half of rate of formation of $\mathrm{H}_2$ or $\mathrm{I}_2$

c) In $\underset{(a q)}{5 \mathrm{Br}^{-}}+\underset{(\mathrm{aq})}{\mathrm{BrO}_3^{-}}+\underset{(\mathrm{aq})}{6 \mathrm{H}^{+}} \rightarrow \underset{(\mathrm{aq})}{3 \mathrm{Br}_2}+3 \mathrm{H}_2 \mathrm{O}(\mathrm{I})$, the rate of consumption of $\mathrm{Br}^{-}(\mathrm{aq})$ is 1.66 times to the rate of a formation of $\mathrm{Br}_2$

Which of the following statements are incorrect?

A zero order reaction is one:

If in the fermentation of sugar in an enzymatic solution that is 0.12 M, the concentration of the sugar is reduced to 0.06 M in 10 h to 0.03 M in 20 h, what is the order of the reaction:

Assertion (A):For a free radical combination, $K=A$.

Reason (R): $E_a$ is zero for free radical combination.

Rate of a chemical reaction becomes 4 times when concentration of reactant is made 4 times. If $50 \%$ of reaction occurs in $1414 \mathrm{sec}$, how long would it take for completion of $75 \%$ reaction?