Chemical kinetics practice · Medium

For the reaction $2 \mathrm{~N}_2 \mathrm{O}_5(\mathrm{~g}) \rightarrow 4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})$ If the concentration of $\mathrm{O}_2$ increases by $2 \times 10^{-3} \mathrm{M}$ in 100 seconds then the rate of disappearance of $\mathrm{N}_2 \mathrm{O}_5$ is :-

For a first order reaction it takes 15 second for 75% completion. The half life of the reaction is

A given sample of milk turns sour at room temperature $\left(27^{\circ} \mathrm{C}\right)$ in $16 \mathrm{~h}.$ In a refrigerator at $7^{\circ} \mathrm{C},$ milk can be stored three times as long before it sours. How long (in hours) it takes for milk to sour at $57^{\circ} \mathrm{C} ?$$(\ln 2=0.7, \ln 3=1.1)$

In general, the rate of a reaction can be increased by all the factors except

Hydrolysis of ethyl acetate is catalysed by acid.

$\mathrm{CH}_3 \mathrm{COOC}_2 \mathrm{H}_5+\mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{H}^{+}} \mathrm{CH}_3 \mathrm{COOH}+\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$

Rate constant of the reaction is $5.56 \times 10^{-6} \mathrm{~s}^{-1}$. What is its rate constant when it is second-order reaction (pseudo unimolecular)?

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

For the second-order reaction ${A}+{B} \rightarrow \text{Products},$ the rate constant $k$, is given as
$k=\frac{2.303}{(a-b) t} \log \frac{b(a-x)}{a(b-x)},$ where, $a$ and $b$ are the initial concentrations of '$A$' and '$B$' and $x$ is the change in concentration after time $t.$ If $b \gg a,$ the reaction reduces to

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

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.

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

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?

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

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

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.