Chemical kinetics practice · Mixed difficulty

Assertion: Hydrolysis of methyl ethanoate is a pseudo first order reaction.

Reason: Water is present in large excess and therefore its concentration remained constant throughout the reaction.

If half life of radioactive bromine ( $\mathrm{Br}-82)$ is $36 \mathrm{hr}$, find percentage remaining after one day. [nearest integer]

What is not correct for a zero order reaction

The half life of a reaction is—of temperature

Half-life of a reaction is found to be inversely proportional to the cube of initial concentration. The order of reaction is

A first order reaction has a specific reaction rate of $10^{-1} \mathrm{~s}^{-1}$. How much time will it take for $100 \mathrm{~g}$ of its reactant to be reduced to $25 \mathrm{~g}$?

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

The rate constant for a first-order reaction is $2.2 \times10^{-5} \mathrm{~s}^{-1}$ at $320^{\circ} \mathrm{C}$. Calculate the time in which the reaction is $15 \%$ complete.

What fraction of a reactant showing first order remains after 40 minute if ${t_{1/2}}$ is 20 minute?

The slope in Arrhenius plot, is equal to:

The reaction obey I order with respect to ${\mathrm{H}_2}$ and $\mathrm{ICl}$ both

${\mathrm{H}_2}\left( \mathrm{g} \right) + 2\mathrm{ICl}\left( \mathrm{g} \right) \to 2\mathrm{HCl}\left( \mathrm{g} \right) + {\mathrm{I}_2}\left( \mathrm{g} \right)$

Which of the following mechanism is in consistent with the given fact?

Mechanism$A:{\mathrm{H}_2}\left( \mathrm{g} \right) + 2\mathrm{ICl} \to 2\mathrm{HCl}\left( \mathrm{g} \right) + {\mathrm{I}_2}\left( \mathrm{g} \right)$

Mechanism$B:\left( \mathrm{i} \right){\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{ICl}\left( \mathrm{g} \right)\xrightarrow{{Slow}}\mathrm{HCl}\left( \mathrm{g} \right) + \mathrm{HI}\left( \mathrm{g} \right)$

$\left( {\mathrm{ii}} \right)\mathrm{HI}\left( \mathrm{g} \right) + \mathrm{ICl}\left( \mathrm{g} \right) \to \mathrm{HCl}\left( \mathrm{g} \right) + {\mathrm{I}_2}$

The half life of a first order reaction is $69.3 \,{sec}$. The value of the rate constant of the reaction is:

For the reaction, ${H_2} + {I_2} \to 2HI$, the differential rate law is

Two substances A and B are present such that $\left[ A \right] = 4\left[ B \right]$ and half-life of $A$ is 5 minute and of $B$ is 15 minute. If they start decaying at the same time following first order, how much time later will the concentration of both of them would be same?

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

The unit of rate constant of second order reaction is

If $'a'$ is the initial concentration of the reactant, the half-life period of the reaction of ${n^{th}}$ order is proportional to

Rate equation for a second order reaction is:

For a first order reaction, the half life period is 5 minutes. The time required for the concentration of the substance to fall from $x\,M\;\,\mathrm{to}\,\,\,\frac{x}{{32}}\,\,M$ is

The activation energy of exothermic reaction $A \to B$ is $80\;kJ\;\mathrm{mo}{\mathrm{l}^{ - 1}}$. The heat of reaction is $200\;kJ\;\;\mathrm{mo}{\mathrm{l}^{ - 1}}$. The activation energy for the reaction $B \to A$ (in $kJ\;\;\mathrm{mo}{\mathrm{l}^{ - 1}})$ will be

$50 \%$ of a first order reaction completes in 20 minute. $100 \%$ of same reaction shall complete in:

The rate of chemical reaction depends on the nature of chemical reactions, because:

A chemical reaction proceeds following formula

$k = PZ\;{e^{ - {E_a}/RT}}$

Which of the following process will increase the rate of reaction?

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

For a given reaction, pressure of catalyst reduces the energy of activation by $2\;\mathrm{k}\;\mathrm{cal }\;\mathrm{at}\;27^\circ C.$ The rate of reaction will be increased by:

Which of the following is not a first order reaction?

The rate constant for the reaction $\mathrm{CO}_2+\mathrm{OH}^{-} \longrightarrow \mathrm{HCO}_3^{-}$ in aqueous solution is $4.0 \times 10^3 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}$ when $\left[\mathrm{CO}_2\right]=10^{-6} \mathrm{~mol} \mathrm{~L}^{-1}$ and $\left[\mathrm{OH}^{-}\right]=0.1 \mathrm{~mol} \mathrm{~L}^{-1}$ Number of moles of $\mathrm{HCO}_3^{-}$formed per second is $x \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$. What is the value of $x$ ?

For the reaction,$C{l_2} + 2{l^ - } \to {I_2} + 2C{l^ - }$ the initial concentration of ${I^ - }$ was $0.20\;mol\;{L^{ - 1}}$ and the concentration after 20 min was $0.18\;mol\;{L^{ - 1}}$.Then the rate of formation of ${I_2}$ in $mol\;{L^{ - 1}}$ would be

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

Half-life of a reaction is found to be inversely proportional to the cube of initial concentration. The order of reaction is