Chemical kinetics practice · Mixed difficulty

The unit of rate constant for a zero order reaction is

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.

Read the following statements.

(i) ${e}^{-{E}_{{a}} / {RT}}$ corresponds to the fraction of molecules that have kinetic energy greater than ${E}_{{a}}$.

(ii) ${E}_{{a}}$ can be calculated as follows

$\log \frac{k_1}{k_2}=\frac{{E}_{{a}}}{2.303 {R}}\left[\frac{{T}_2-{T}_1}{{~T}_1 {~T}_2}\right]$

(iii) Catalyst can alter a reaction both ways means it can either decrease on increase rate of reaction

(iv) A catalyst always decreases the activation energy of the reaction but does not alter Gibb's energy.

(v) A catalyst does not alter equilibrium constant rather, it helps in attaining the equilibrium faster.

Which of the following is the correct codes for above statements ?

For the first order reaction ${t_{\mathrm{av}}}$ (average life), ${t_{\frac{1}{2}}}\,\,\,\,\mathrm{and}\,\,\,\,{t_{\frac{3}{4}}}$ in the increasing order are

The branch of chemistry which deals with the reaction rates and reaction mechanism is called:

The Arrhenius equation expressing the effect of temperature on the rate constant of reaction is:

Which of the following statements are incorrect?

For the first-order reaction with $C_0$ as the initial concentration and $C$ at time $t,\left(C_0-C\right)=$

Which one of the following is wrongly matched?

A first order reaction has the rate constant, ${k}=4.6 \times 10^{-3} \, \mathrm{s}^{-1}$. The number of correct statement/s from the following is/are _____

Given: $\log 3=0.48$
A. Reaction completes in $1000 \, \mathrm{s}$.
B. The reaction has a half-life of $500 \, \mathrm{s}$.
C. The time required for $10 \%$ completion is 25 times the time required for $90 \%$ completion.
D. The degree of dissociation is equal to $\left(1-e^{-k t}\right)$
E. The rate and the rate constant have the same unit.

The initial rates of reaction $3 \mathrm{A}+2 \mathrm{B}+\mathrm{C} \longrightarrow$ Products, at different initial concentrations are given below:

$\begin{array}{cccccccccccccccccccc} {{\text{Initial rate,}}}&{{{\left[ {\text{A}} \right]}_0},{\text{M}}}&{{{\left[ {\text{B}} \right]}_0},{\text{M}}}&{{{\left[ {\text{C}} \right]}_0},{\text{M}}} \\ {{\text{M}}{{\text{s}}^{ - 1}}}&{}&{}&{} \\ {5.0 \times {{10}^{ - 3}}}&{0.010}&{0.005}&{0.010} \\ {5.0 \times {{10}^{ - 3}}}&{0.010}&{0.005}&{0.015} \\ {1.0 \times {{10}^{ - 2}}}&{0.010}&{0.010}&{0.010} \\ {1.25 \times {{10}^{ - 3}}}&{0.005}&{0.005}&{0.010} \end{array}$

The order with respect to the reactants, $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ are respectively

If the rate of reaction $A \to B$ doubles on increasing the concentration of A by 4 times, the order of the reaction is

The chemical reaction $2{\mathrm{O}_3} \to 3{\mathrm{O}_2}$ proceeds as follows

${\mathrm{O}_3}\;\leftrightharpoons\;{\mathrm{O}_2} + \mathrm{O}(fast)$

$\mathrm{O} + {\mathrm{O}_3} \to 2{\mathrm{O}_2}(slow)$

The rate law expression should be

The rate at which a substance reacts depends on its

The activation energies of two reactions are ${E_a}$ and ${E'_a}$ with ${E_a} > {E'_a}.$ If the temperature of the reacting systems is increased from ${T_1}$ to ${T_2}$, predict which alternative is correct. $K'$ are rate constants at higher temperature. Assume $A$ being same for both the reactions:

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

In the following reaction; $xA \to yB$
${\log _{10}}\left[ { - \frac{{d\left[ A \right]}}{{dt}}} \right] = {\log _{10}}\left[ {\frac{{d\left[ B \right]}}{{dt}}} \right] + 0.3010$ A and B respectively can be

For a chemical reaction $2X + Y \to Z$, the rate of appearance of $Z\;is\;0.05\;\mathrm{mol}\;{\mathrm{L}^{ - 1}}\mathrm{.}$ The rate of disappearance of $X$ will be

Effective collisions are known to possess:

A. energy greater than threshold energy.

B. breaking of old bond in reactant.

C. formation of new bond in product.

D. high activation energy.

E. proper orientation.

The incorrect statement is:

For a first order reaction ${X_{\left( g \right)}} \to {Y_{\left( g \right)}} + {Z_{\left( g \right)}}$. The half – life period is 6.93 min. The time required for the completion of 99% of the chemical reaction will be

For the reaction, $2N{H_3}(g) \to {N_2}(g) + 3{H_2}(g) ,- \frac{{d\left[ {N{H_3}} \right]}}{{dt}} = {K_1}\left[ {N{H_3}} \right]$; $\frac{{ + d\left[ {{N_2}} \right]}}{{dt}} = {K_2}\left[ {N{H_3}} \right];\frac{{ + d\left[ {{H_2}} \right]}}{{dt}} = {K_3}\left[ {N{H_3}} \right];$ the relation between ${K_1},{K_2}$ and ${K_3}$ is

The half time of a second order reaction is:

If, at $\mathrm{t}=30 \mathrm{~sec},[\mathrm{A}]=100 \mathrm{~moles} / \mathrm{L}$,

at $\mathrm{t}=40 \mathrm{~sec},[\mathrm{A}]=80 \mathrm{~moles} / \mathrm{L}$,

at $\mathrm{t}=50 \mathrm{~sec},[\mathrm{A}]=64 \mathrm{~moles} / \mathrm{L}$

For a reaction, $A \rightarrow B$, the order will be

Fraction of molecule having energy greater or equal to activation energy $E_a$ at temperature $T K$ is given by

The inversion of Cane sugar proceeds with constant halflife of 500 minutes at $\mathrm{p}^{\mathrm{H}}=5$ for any concentration of sugar. However if $\mathrm{p}^{\mathrm{H}}=6$, the half-life changes to 50 minutes. For this reaction rate equation is rate $=\mathrm{k}$ [sugar $^{\mathrm{m}}\left[\mathrm{H}^{+}\right]^{\mathrm{n}}$. The value of'n" is

For a reversible reaction $A \rightleftharpoons B$, the $\Delta \mathrm{H}_{\text {forward reaction }} =20 \, \mathrm{kJ} \, \mathrm{mol}^{-1}$. The activation energy of the uncatalyzed forward reaction is $300 \, \mathrm{kJ} \, \mathrm{mol}^{-1}$. When the reaction is catalysed keeping the reactant concentration same, the rate of the catalysed forward reaction at $27^{\circ} \mathrm{C}$ is found to be same as that of the uncatalyzed reaction at $327^{\circ} \mathrm{C}$. The activation energy of the catalysed backward reaction is _____ $\mathrm{kJ} \, \mathrm{mol}^{-1}$.

Which is correct about zero order reaction?

A first order reaction is 75% complete after 32 min. when was 50% of the reaction completed?

The unit and value of rate constant and that of rate of reaction are same for

Mathematical expression for ${t_{1/4}}$ i.e., when ${\left( {1/4} \right)^{th}}$ reaction is over following first order kinetics can be given by