Chemical kinetics practice · Mixed difficulty

Find the two third life $\left( {{t_{1/2}}} \right)$ of a first order reaction in which $k = 5.48 \times {10^{ - 14}}$ per second

The activation energies of two reactions are ${E_1}\;and\;{E_2}({E_1} > {E_2})$. If the temperature of the system is increased from ${T_1}\;and\;{T_2}$, the rate constant of the reactions changes from ${k_1}\;to\;{k_2}$ in the first reaction and ${k_1}\;and\;{k_2}$ in the second reaction. Predict which of the following expression is correct?

Which of the following statement is true for the reaction, ${H_2} + B{r_2} \to 2HBr$. The rate law is $\frac{{dx}}{{dt}} = K\left[ {{H_2}} \right]{\left[ {B{r_2}} \right]^{1/2}}$

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?

A first order reaction is 10% complete in 20 min. The time taken for 19% completion is

The following statement(s) is (are) correct :

(i) A plot of $\log k_p$ versus $1 / T$ is linear

(ii) A plot of $\log [\mathrm{X}]$ versus time is linear for a first order reaction, ${X} \rightarrow {P}$

(iii) A plot of log p versus $1 / {T}$ is linear at constant volume

(iv) A plot of ${p}$ versus $1 / {V}$ is linear at constant temperature

For an elementary reaction $2A + 3B2C$ . The rate of disappearance of B is

The temperature coefficient of most of the reactions lies between

The rate of a reaction is doubled when temperature increases by $10^\circ C$. If temperature is increased by $100^\circ C$, then rate of reaction will become

In a second order reaction when the concentration of both reactant are equal, the reaction is completed in 500 s. How long will it take for the reaction to go to 60% completion?

Which of the following is the correct statement?

Assertion (A):The instantaneous rate of reaction can be studied in chemical kinetics.

Reason (R): Ionic reactions occur instantaneously.

Effect of temperature on reaction rate is given by

The inversion of cane sugar proceeds with half-life of 500 minute at $\mathrm{pH}=5$ for any concentration of sugar. However, if $\mathrm{pH}=6,$ the half-life changes to 50 minute. The rate law expression for the sugar inversion can be written as

The slope in Arrhenius plot, is equal to:

${t_{1/4}}\;$ can be taken as the time taken for the concentration of reactant to drop to ${\frac{3}{4}}$ of its initial value. If the rate constant for a first order reaction is $k$ the ${t_{1/4}}\;$ can be written as

Consider the reaction $2A + B \to product$
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is

For a first reaction; $2A\left( g \right) \to 2B\left( g \right) + C\left( g \right)$, the initial pressure is ${P_0}$ and after time $'t'$, total pressure of reaction mixture becomes ${P_t}$, the rate constant is

The rate constants ${K_1}$ and ${K_2}$ for two different reactions are ${10^{16}}{e^{ - 2000/T}}$ and ${10^{15}}{e^{ - 1000/T}}$, respectively. The temperature at which${K_1} = {K_{2\;}}$ is:

A reaction was observed for 15 days and the percentage of the reactant remaining after the days indicated was recorded in the following table.

Time ( days ) % Reactant remaining 0 100 2 50 4 39 6 25 8 21 10 18 12 15 14 12.5 15 10 $\;\;\begin{array}{llllllllllllllllllll} {\mathbf{Time}\mathrm{ }\left( {\mathbf{days}} \right)\;\;\;\;\;\% \mathrm{ }\mathbf{Reactant}\mathrm{ }\mathbf{remaining}}\\ {\;\;\;\;\;\;0\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;100}\\ {\;\;\;\;\;2\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;50}\\ {\;\;\;\;\;4\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;39}\\ {\;\;\;\;\;6\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;25}\\ {\;\;\;\;\;8\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;21}\\ {\;\;\;\;10\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;18}\\ {\;\;\;\;12\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;15}\\ {\;\;\;\;14\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;12.5}\\ {\;\;\;\;15\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;10} \end{array}$
Which one of following best describes the order and the half-life of the reaction?

Reaction order Half-life (days)

In the reaction; $A + 2B \to 3C + D$ which of the following expressions does not describe changes in the concentration of various species as a function of time?

Activation energy of a reaction

The differential rate expression for the reaction ${\mathrm{H}_2} + {\mathrm{I}_2} \to 2\mathrm{HI}$ is:

A reaction, ${A_2} + {B_2} \to 2AB$ occurs by the following mechanism;
${A_2} \to A + A$ ……(Slow)
$A + {B_2} \to AB + B$ …..(Fast)
$A + B \to AB$ ......(Fast)
Its order would be:

For the non-equilibrium process, $A + B \to products$, the rate is first order with respect to $A$ and second order respect to $B$. If $1.0\;mole$ each of $A$ and $B$ are introduced into a 1 litre vessel and the initial rate was $1.0 \times {10^{ - 2}}\;\mathrm{mol}/\mathrm{litre}\;\;\mathrm{sec}\mathrm{.}$ The rate (in $\mathrm{mol}\;\mathrm{litr}{\mathrm{e}^{ - 1}}{\sec ^{ - 1}}$ ) when half of the reactants have been used:

The rate of the reaction

$\mathrm{CC}{\mathrm{l}_3}\mathrm{CHO} + \mathrm{NO} \to \mathrm{CHC}{\mathrm{l}_3} + \mathrm{NO} + \mathrm{CO}$ is equal to rate $k\left[ {\mathrm{CC}{\mathrm{l}_3}\mathrm{CHO}} \right]\left[ {\mathrm{NO}} \right]$.

If concentration is expressed in mol/L. The unit of k is

It takes 40 minutes for the completion of $50 \%$ of the reaction $\mathrm{A} \rightarrow \text{Products}.$ For the completion of next $50 \%$ of the reaction, the time taken is 80 minutes. The order of the reaction is