Chemical kinetics practice · Easy

In the reaction $A + B \to products$, if B is taken in excess, then it is an example of

Which of the following statement is incorrect about the molecularity of a reaction?

The unit of rate constant for a zero order reaction is

For $A + B \to C + D,\;\Delta H = - 20\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$ the activation energy of the forward reaction is $85\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}.$ The activation energy for backward reaction is …$\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$.

The rate constant ${K_1}$ of a reaction is found to be double that of rate constant ${K_2}$ of another reaction. The relationship between corresponding activation energies of the two reactions at same temperature $({E_1}\;and\;{E_2})$ can be represented as:

Calculate the overall order of a reaction which has the rate expression

(a) Rate $=k[\mathrm{~A}]^{1 / 2}[{~B}]^{3 / 2}$

(b) Rate $=k[\mathrm{~A}]^{3 / 2}[{~B}]^{-1}$

The given reaction,

$2\mathrm{FeC}{\mathrm{l}_3} + \mathrm{SnC}{\mathrm{l}_2} \to \mathrm{SnC}{\mathrm{l}_4} + 2\mathrm{FeC}{\mathrm{l}_2}$ is an example of:

During a particular reaction $20 \%$ of the reactant decomposes in $1 \mathrm{~h},\,40 \%$ in $2 \mathrm{~h}, 60 \%$ in $3 \mathrm{~h}$ and so on. The unit of rate constant is

Which of the following is an incorrect statement about first-order reaction?

In Arrhenius equation $K = A\;{e^{ - {E_a}/RT}}$, the quantity $- {E_a}/RT$ is referred as:

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

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

The slope in Arrhenius plot, is equal to:

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

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

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 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?

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:

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

For the elementary step,

${\left( {\mathrm{C}{\mathrm{H}_3}} \right)_3} \cdot \mathrm{CBr}\left( {aq} \right) \to {\left( {\mathrm{C}{\mathrm{H}_3}} \right)_3}{\mathrm{C}^ + }\left( {aq} \right) + \mathrm{B}{\mathrm{r}^ - }\left( {aq} \right)$ the molecularity is:

The decomposition of phosphine $\mathrm{(P}{\mathrm{H}_\mathrm{3}}\mathrm{)}$ on tungsten at low pressure is a first – order reaction. It is because the

A reaction involving two different reactants can never be

For $A + B \to C + D,\;\Delta H = - 20\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$ the activation energy of the forward reaction is $85\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}.$ The activation energy for backward reaction is …$\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$.

For the reaction, ${\mathrm{N}_2}{\mathrm{O}_5} \to 2\mathrm{N}{\mathrm{O}_2} + \frac{1}{2}{\mathrm{O}_2}$

Given, $- \frac{{d\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]}}{{dt}} = {K_1}\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]$

$\frac{{d\left[ {\mathrm{N}{\mathrm{O}_2}} \right]}}{{dt}} = {K_2}\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]$

$\mathrm{and}\;\;\frac{{d\left[ {{\mathrm{O}_2}} \right]}}{{dt}} = {K_3}\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]$

The relation in between ${K_1},{K_2}\;and\;{K_3}$ is:

The decomposition of phosphine $\left( {P{H_3}} \right)$ on tungsten at low pressure is a first order reaction. If is because the

The rate law of the reaction,

$A + 2B \to \mathrm{Product}\mathrm{.}$

Product is given by $\frac{{d\left[ P \right]}}{{dt}} = K{\left[ A \right]^2} \cdot \left[ B \right].$. If $A$ is taken in large excess, the order of the reaction will be: