Chemical kinetics practice · Mixed difficulty

The integrated rate equations can be determined for

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

When concentration of the reactant $A$ in the reaction $A \to B$ increases to 8 times, then rate increases to 2 times only. The order of reaction is

The half-life for the first-order decomposition of nitramide $\mathrm{NH}_4 \mathrm{NO}_2(\mathrm{aq}) \rightarrow \mathrm{N}_2 \mathrm{O}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}({l})$ is 123 minutes at $27^{\circ} \mathrm{C}$. If $200 \mathrm{~ml}$ of $0.02 \mathrm{~M}$ $\mathrm{NH}_4 \mathrm{NO}_2$ solution is allowed to decompose, then how long must the reaction proceed to produce $49.26 \mathrm{~ml}$ of 'wet' $\mathrm{N}_2 \mathrm{O}(\mathrm{g})$ measured at $27^{\circ} \mathrm{C}$ and $785 \mathrm{~mm} \mathrm{~Hg}?$ The vapour pressure of water at $27^{\circ} \mathrm{C}$ is $25 \mathrm{~mm} \mathrm{~Hg}$.

The concentration of R in the reaction $R \to P$ was measured as a function of time and the following data is obtained
$\begin{array}{llllllllllllllllllll} {\left[ R \right]\left( {molar} \right)\;\;\;1.00\;\;\;\;\;\;0.75\;\;\;\;\;0.40\;\;\;\;\;0.10}\\ {t\;\left( {min} \right)\;\;\;\;\;\;\;\;\;0.00\;\;\;\;\;0.05\;\;\;\;\;0.12\;\;\;\;\;0.18} \end{array}\;$
The order of the reaction is

The energy of activation of reaction, if its rate double when the temperature is raised from $290 \mathrm{~K}$ to $300 \mathrm{~K}$ is $\mathrm{x}$ kcal then the value of $\mathrm{x} / 3$ is (Take $\mathrm{R}=2 \mathrm{cal} / \mathrm{k} / \mathrm{mol}$ )

For the reaction $2A + B \to 3\,C + D$, which of the following does not express the reaction rate

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)

For the consecutive first-order reactions $\mathrm{A} \xrightarrow{K_{\mathrm{1}}}\mathrm{B} \xrightarrow{K_2} \mathrm{C}, \mathrm{B}$ is in steady state. What will be the concentration of $\mathrm{C}$ at this stage? At $t=0,[\mathrm{A}]=[\mathrm{A}]_0$ and $[\mathrm{B}]=[\mathrm{C}]=0$.

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

Reason (R): Ionic reactions occur instantaneously.

For the reaction,

$2{N_2}{O_5}\left( g \right) \to 4N{O_2}\left( g \right) + {O_2}\left( g \right)$

If the concentration of $N{O_2}$ increase by $5.2 \times {10^{ - 3}}\;M$ in 100 s then the rate of the reactions

The unit of rate constant obeying the rate expression $r = k{\left[ A \right]^1}{\left[ B \right]^{2/3}}$ is

Which of the following expression is correct for second order reaction. (${C_0}$ refers to initial concentration of reactant)?

Assertion (A):Larger is the activation energy, lesser is the effect of a given temperature rise on rate constant $K.$

Reason (R): $K=A e^{-E_a / R T}$

For the consecutive first-order reactions: ${A} \xrightarrow{K_1} {B} \xrightarrow{K_2} {C},$
in what condition, $[{C}]=\left[{A}_0\right] .\left(1-e^{-K_1 t}\right)?$

The rate of a chemical reaction doubled for every $10^\circ C$ rise in temperature. If the temperature is increased by $60^\circ C$ the rate of reaction increase by

Activation energy of a chemical reaction can be determined by

The rate of reaction $2 \mathrm{X}+\mathrm{Y} \rightarrow$ Products is given by $\frac{\mathrm{d}[\mathrm{Y}]}{\mathrm{d} t}=k[\mathrm{X}]^2[\mathrm{Y}]$, if $\mathrm{X}$ is present in large excess, the order of the reaction is

With the help of following reactions, arrange metals A, B, D and E in decreasing order of their reactivity ?

(a) $B +{ANO}_3 \rightarrow {BNO}_3+ A$

(b) $A +{HCl} \rightarrow {ACl}+\frac{1}{2} {H}_2$

(c) $D +{ECl} \rightarrow {DCl}+ E$

(d) $D +{HNO}_3 \rightarrow$ No reaction

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)$

Rate constant of the following reaction is $1.0 \times 10^{-5} \mathrm{~s}^{-1}$.

$2 \mathrm{~N}_2 \mathrm{O}_5 \longrightarrow 2 \mathrm{~N}_2 \mathrm{O}_4+\mathrm{O}_2$

At a time when $\left[\mathrm{N}_2 \mathrm{O}_5\right]=0.2 \mathrm{~mol} \mathrm{~L}^{-1}$, average rate of the reaction

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

The reaction of hydrogen and iodine monochloride is given as:

${H}_2({~g})+2 {ICl}({g}) \longrightarrow 2 {HCl}({g})+{I}_2({~g})$

The reaction is of first order with respect to ${H}_2({~g})$ and ${ICI}({g})$, following mechanisms were proposed.

Mechanism A:

${H}_2({~g})+2 {ICl}({g}) \longrightarrow 2 {HCl}({g})+{I}_2({~g})$

Mechanism B:

$\begin{aligned} & {H}_2({~g})+{ICl}({g}) \longrightarrow {HI}({g}) ; \text { slow } \\ & {HI}({g})+{ICl}({g}) \longrightarrow {HCl}({g})+{I}_2({~g}) ; \text { fast } \end{aligned}$

Which of the above mechanism(s) can be consistent with the given information about the reaction?

In a reaction $A + B \to C$, the rate expression is $R = k\left[ A \right]{\left[ B \right]^2}$ If the concentration of both the reaction is doubled at constant volume then the rate of the reaction will be

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

Which of the following statements is not correct?

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