Chemical kinetics practice · Mixed difficulty

The rate of the reaction $3 \mathrm{A}+2 \mathrm{B} \rightarrow \text{Products}$ is given by the rate expression rate $=K[\mathrm{A}][\mathrm{B}]^2.$ If $\mathrm{A}$ is taken in large excess, then the reaction start obeying

In a reaction for every $10^{\circ} \mathrm{C}$ rise of temperature, the rate is tripled. If the temperature is increased from $10^{\circ} \mathrm{C}$ to $50^{\circ} \mathrm{C}$, the rate of the reaction will become

Half-life of two samples is 0.1 and 0.8 s. Their respective concentration is 400 and 50 respectively.

The order of reaction is

Assertion (A):A plot of $\log \frac{d X}{d t} \text{ vs. }\log (a-x)$ leads to value of $K$ as antilog (intercept) and slope equal to order of reaction.

Reason (R):$\frac{d X}{d t}=K(a-x)^n$

Statement I Kinetics of study of decomposition of $\mathrm{N}_2 \mathrm{O}_5(g)$ to $\mathrm{NO}_2(g)$ and $\mathrm{O}_2(g)$ can be studied by measuring pressure of $\mathrm{O}_2$ gas in $\mathrm{CCl}_4$ solvent.

$2 \mathrm{~N}_2 \mathrm{O}_5(g) \longrightarrow 4 \mathrm{NO}_2(g)+\mathrm{O}_2(g)$

Statement II At the start, volume of $\mathrm{O}_2(g)$ is zero.

For a reaction scheme, $A\xrightarrow{{{k_1}}}B\xrightarrow{{{k_2}}}C,$ if the rate of formation of $B$ is set to be zero then the concentration of B is given by

The rate constant of a first order reaction is $3 \times {10^{ - 6}}$ per second and initial concentration is $0.10\;\mathrm{ }M.$ Then the initial rate of reaction is

Two radio isotopes ${P}$ and ${Q}$ of atomic mass 10 and 20 respectively are mixed in equal amount by mass. After 20 days, their weight ratio $\frac{{W}_{{P}}}{{W}_{{Q}}}$ is found to be $1: 4$. Isotope ${Q}$ has a half-life of 10 days. The half-life of isotope ${P}$ is:

The rate equation for the reaction $2A + B \to C$ is found to be
$Rate = k\left[ A \right]\left[ B \right]$
The correct statement in relation to this reaction that the

For the first-order parallel reactions $\mathrm{A} \xrightarrow{K_1} \mathrm{B}$ and $\mathrm{A} \xrightarrow{K_2} \mathrm{C}, K_1=8 \mathrm{~min}^{-1}$ and $K_2=2 \mathrm{~min}^{-1}$ at $300 \mathrm{~K}.$ If the activation energies for the formation of $\text{B}$ and $\text{C}$ are $20$ and $28.314 \mathrm{~kJ} / \mathrm{mol},$ respectively, then find the temperature at which $\text{B}$ and $\text{C}$ will be obtained in $2: 1$ mole ratio. $(\ln 2=0.7)$

The decomposition of ${N}_2 {O}_5$ is a first order reacton represented by ${N}_2 {O}_5 \longrightarrow {N}_2 {O}_4+\frac{1}{2} {O}_2$. After 15 minutes the volume of ${O}_2$ produced is $9 \, \mathrm{ml}$ and at the end of the reaction $35 \mathrm{~mL}$. The rate constant it equal to

Which of the following represents the expression for $3 / 4$th the life of a first-order reaction?

Timetaken for $12.8 {~g}$ of a radioactive substance to decay to $0.4 {~g}$ is: (half life is $138 {~s}$ )

Which of the following rate law has an overall order of 0.5 for reaction involving substances $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ ?

${t_{99.9\% }}$ of a first order reaction is 100 minutes. Rate constant of the reaction is

Which of the following statement is not correct for the reaction: $4A + B \to 2C + 2D$

Consider the following statements,

The rate law for the acid catalysed hydrolysis of an ester being given as

$Rate = k\;\left[ {{H^ + }} \right]\;\left[ {ester} \right] = k'\;\left[ {ester} \right]$

If the acid concentration is doubled at constant ester concentration

1. The second order rate constant, $k$ is doubled.

2. The pseudo first order rate constant, $k$ is double.

3. The rate of the reaction is doubled.

Which of the above statements are correct?

How much faster would a reaction proceed at $25^\circ C$ than at $0^\circ C$ if the activation energy is $65\;kJ?$

For the reaction system

$2\mathrm{NO}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right) \to 2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)$ if the volume of the reaction vessel is reduced to one-third of its original volume, what will be the order of the reaction?

DDT on exposure to water decomposes. Half-life is 10 yr. How much time it will take for its decomposition to 99%?

For the reaction $\mathrm{A} \xrightarrow{K_1} \mathrm{B} \xrightarrow{K_2} \mathrm{C} \xrightarrow{K_3} \mathrm{D},$ where $K_3>K_2>K_1;$ the rate of formation of $\mathrm{D}$ is determined by

The minimum energy required for the reacting molecules to undergo reaction is :

For the reaction $2{N_2}O5 \to 4N{O_2} + {O_2}$ rate and rate constant are $1.02 \times {10^{ - 4}}\,\,mol.{L^{ - 1}}.{\sec ^{ - 1}}$ and $3.4 \times {10^{ - 5}}{\sec ^{ - 1}}$ respectively then concentration of ${N_2}{O_5}$ at that time will be

Half life of a first order reaction is $4 {~s}$ and the initial concentration of the reactant is $0.12 {M}$. The concentration of the reactant left after $16 {~s}$ is

Consider the following statements

a) Increase in concentration of reactant increases the rate of zero order reaction

b) Rate constant K is equal to collision frequency A if ${E_a} = 0$

c) Rate constant K is equal to collision frequency A if ${E_a} = \, \propto$

d) ln K Vs T is a straight line

e) ln K Vs 1/T is a straight line

Correct statements are

The rate constant of a first order reaction at $27^\circ \,C$ is ${10^{ - 3}}\,\mathrm{mi}{\mathrm{n}^{ - 1}}$. The temperature coefficient of this reaction is 2. What is the rate constant (in $\mathrm{mi}{\mathrm{n}^{ - 1}}$) at $17^\circ \,C$ for this reaction?

If for a radio-isotope, at the end of 4.2 days, ${N}=0.798 {~N}_0$. What will be half life period of its nucleus?

The ratio of $\frac{{ }^{14} \mathrm{C}}{{ }^{12} \mathrm{C}}$ in a piece of wood is $\frac{1}{8}$ part that of atmosphere. If half life of ${ }^{14} \mathrm{C}$ is 5730 years, the age of wood sample is …..years.

Statement I A high activation energy corresponds to a
reaction rate that is very sensitive to temperature.
Statement II In following gaseous phase reaction $\mathrm{CH}_3+\mathrm{CH}_3 \longrightarrow \mathrm{CH}_3-\mathrm{CH}_3$ rate is independent of temperature.

In the reaction
$BrO_3^ - \left( {aq} \right) + 5\,B{r^ - }\left( {aq} \right) + 6{H^ + }\left( {aq} \right) \to 3B{r_2}\left( l \right) + 3{H_2}O\left( l \right)$
The rate of appearance of bromine $\left( {B{r_2}} \right)$ is related to rate of disappearance of Bromide ions is