Chemical kinetics practice · Mixed difficulty

The rate for the reaction, $RCl + NaOH\left( {aq} \right) \to ROH + NaCl$ is given by $rate\mathrm{ } = K_1\left[ {RCl} \right].$ The rate of the reaction is

In gaseous reactions important for the understanding of the upper atmosphere ${\mathrm{H}_2}\mathrm{O}$ and $\mathrm{O}$ react bimolecularly to form two $\mathrm{OH}$ radicals. $\Delta H$ for this reaction is $72\;\mathrm{kJ}\;\mathrm{ at}\;500\;\mathrm{K}$ and ${E_a}$ is $77\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$, then ${E_a}$ for the bimolecular recombination of two OH radicals to form ${\mathrm{H}_2}\mathrm{O}$ and $\mathrm{O}$ is:

The half life for a reaction … of temperature.

For irreversible elementary reactions in parallel ${A}\xrightarrow{K_1} {R}$ and ${A} \xrightarrow{K_2} {S},$ the rate of disappearance of reactant '${A}$' is

In Arrhenius equation, the fraction of effective collisions is given by

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?

Effective collisions are those in which molecules must:

The inversion of cane sugar into glucose and fructose is:

What is the activation energy for a reaction if its rate doubles when the temperature is raised from $20^{\circ} \mathrm{C}$ to $35^{\circ} \mathrm{C}$? $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

A first order reaction is 20% complete in 10 min. What is the rate constant of the reaction?

At room temperature, the reaction between $\mathrm{NO}$ and ${\mathrm{O}_2}$ to give $\mathrm{N}{\mathrm{O}_2}$ is fast, while that between $\mathrm{CO}$ and ${\mathrm{O}_2}$ is slow. It is due to:

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

For a first order reaction the plot of $\log [A]_t$ vs $t$ is linear with a

For a reaction of order $n$, the unit of the rate constant is

What is the formula to find value of ${t_{1/2}}$ for a zero order reaction?

Which of the following does not affect the rate of reaction?

The reaction $2A + B + C \to D + E$ is found to be first order in $A$, second in $B$ and zero order in $C$. What is the effect on the rate of increasing concentration of $A$, $B$ and $C$ two times?

Which of the following theory is not related to chemical kinetics?

What is the activation energy (KJ/mole) for a reaction if it is rate constant doubles when the temperature is raised from 300K to 400K? $\left[ {R = 314J\,mol.{K^{ - 1}}} \right]$

Which statement is correct?

If $a$ is the initial concentration of the reactant and $(a-$ $x)$ is the concentration at time $t$ for the first-order reaction (rate constant $k$). Then which of the following statements are correct.

(I) $x=a\left(1-e^{k_1 t}\right)$

(II) $(a-x)=a\left(\frac{1}{2}\right)^y$ where $y=\frac{t}{t_{50}}$

(III) $k_1=\frac{2.303}{t} \log \left(\frac{a}{a-x}\right)$

Which one is not correct?

Read the following statements

(i) Order of reaction can be fractional or zero.

(ii) Molecularity of a reaction can be fractional but cannot be zero.

(iii) Slowest step in the complex reaction is considered as a rate determining step.

(iv) Units of rate constant for second order reaction are ${mol}\, {L} \,{s}{ }^{-1}$.

(v) Order is applicable to elementary as well as complex reactions whereas molecularity is applicable only for elementary reactions.

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

The rate law for a reaction between the substances $A$ and $B$ is given by $rate = k{\left[ A \right]^n}{\left[ B \right]^m}$. On doubling the concentration of $A$ and halving the concentration of $B$, the ratio of the new rate to the earlier rate of the reaction will be as

Rate constant for a reaction is $\lambda$. Average life is represent by

$2{N_2}{O_5}\;\leftrightharpoons\;4N{O_2} + {O_2}$

For the above reaction which of the following is not correct above rates of reaction?

The rate constant of a reaction at temperature $200\;K$ is 10 times less than the rate constant at $400\;K$. What is the activation energy (${E_a}$ ) of the reaction?

For the chemical reaction ${A} \rightarrow \text{products},$ the rate of disappearance of ${A}$ is a given by

$r_{{A}}=-\frac{{d} C_{{A}}}{{d} t}=\frac{K_1 \cdot C_{{A}}}{1+K_2 \cdot C_{{A}}}$

At low concentration of ${A},$ expressed as $C_{{A}},$ the reaction is of the first-order with the rate constant

For the reaction ${N_2}{O_5}(g) \to 2N{O_2}(g)\; + \;\frac{1}{2}{O_2}(g),$ the rate of disappearance of ${N_2}{O_5}$ is $6.25 \times {10^{ - 3}}\;\mathrm{mol}\;{\mathrm{L}^{ - 1}}\;{\mathrm{s}^{ - 1}}.$ The rate of formation of $N{O_2}$ and ${O_2}$ will be respectively.

The following homogeneous gaseous reactions were experimentally found to be second order overall.

$1.\;2\mathrm{NO} \to {\mathrm{N}_2} + {\mathrm{O}_2}$

$2.\;3{\mathrm{O}_2} \to 2{\mathrm{O}_3}$

$\mathrm{3}\mathrm{.}\;{\mathrm{N}_2}{\mathrm{O}_3} \to \mathrm{NO} + \mathrm{N}{\mathrm{O}_2}$

$\mathrm{4}\mathrm{.}\;{\mathrm{H}_2} + {\mathrm{I}_2} \to 2\mathrm{HI}$

Which of these are most likely to be elementary reaction that occur in one step?