Chemical Kinetics

For an elementary chemical reaction, the Arrhenius plot is given below.
If the energy of activation is $6.64 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\mathrm{R}=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, the temperature at which the...

$2 A \xrightarrow{k} B$ is a zero-order reaction, where $k=1.0 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$. If the initial concentration of $A$ is 2 M , then the time taken to complete $75 \%$ of the reaction will be

For a certain reaction $R \rightarrow$ Product, the plot of concentration $[R]$ vs time has a negative slope as shown. The order of reaction is :

Given below is an expression for the rate constant of a first-order reaction occurring at a certain temperature, $\mathrm{T}(\mathrm{K})$.
\(\operatorname{lnk}=14.34-\frac{1.25 \times 10^4}{T}\)
The energy of activation in $\mathrm{kcal} ...

\(\text { Match List I with List II : }\)
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;wor...

If the half-life ( $t_{1 / 2}$ ) for a first order reaction is 1 minute, then the time required for $99.9 \%$ completion of the reaction is closest to :

If the rate constant of a reaction is $0.03 \mathrm{~s}^{-1}$, how much time does it take for $7.2 \mathrm{~mol} \mathrm{~L}^{-1}$ concentration of the reactant to get reduced to $0.9 \mathrm{~mol} \mathrm{~L}^{-1}$ ?
(Given: $\log 2=0.301$...

Rate constants of a reaction at \(500 \mathrm{~K}\) and \(700 \mathrm{~K}\) are \(0.04 \mathrm{~s}^{-1}\) and \(0.14 \mathrm{~s}^{-1}\), respectively; then, activation energy of the reaction is :
(Given: $$\log 3.5=0.5441, \mathrm{R}=8.31 \...

Which of the following plot represents the variation of \(\ln \mathrm{k}\) versus \(\frac{1}{\mathrm{~T}}\) in accordance with Arrhenius equation?

Following data is for a reaction between reactants A and B :

.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;pa...

Which plot of \(\ln \mathrm{k}\) vs \(\frac{1}{\mathrm{~T}}\) is consistent with Arrhenius equation?

The rate of a reaction quadruples when temperature changes from \(27^{\circ} \mathrm{C}\) to \(57^{\circ} \mathrm{C}\). Calculate the energy of activation.
Given $$\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \log 4=0.6...

Activation energy of any chemical reaction can be calculated if one knows the value of

The correct options for the rate law that corresponds to overall first order reaction is

For a reaction \(3 \mathrm{~A} \rightarrow 2 \mathrm{~B}\)
The average rate of appearance of \(\mathrm{B}\) is given by \(\frac{\Delta[B]}{\Delta t}\). The correct relation between the average rate of appearance of \(\mathrm{B}\) with the a...

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R.
Assertion A : A reaction can have zero activation energy.
Reason R : The minimum extra amount of energy absorbed by reactant molecules so ...

For a certain reaction, the rate \(=\mathrm{k}[\mathrm{A}]^{2}[\mathrm{~B}]\), when the initial concentration of A is tripled keeping concentration of \(\mathrm{B}\) constant, the initial rate would

For a chemical reaction
4A + 3B \(\to\) 6C + 9D
Rate of formation of C is 6 \(\times\) 10\(-\)2 mol L\(-\)1 s\(-\)1 and rate of disappearance of A is 4 \(\times\) 10\(-\)2 mol L\(-\)1 s\(-\)1. The rate of reaction and amount of B consumed i...

For a first order reaction A \(\to\) Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min\(-\)1 is

The given graph is a representation of kinetics of a reaction

The y and x axes for zero and first order reactions, respectively are

The slope of Arrhenius plot \(\left( {\ln \,k\,v/s{1 \over T}} \right)\) of first order reactino is \(-\)5 \(\times\) 103K. The value of Ea of the reaction is. Choose the correct option for your answer.[Given R = 8.314 JK\(-\)1mol\(-\)1]

For a reaction, A \(\to\) B, enthalpy of reaction is \(-\)4.2 kJ mol\(-\)1 and enthalpy of activation is 9.6 kJ mol\(-\)1. The correct potential energy profile for the reaction is shown in option.

The rate constant for a first order reaction is 4.606 \(\times\) 10-3 s-1. The time required to reduce 2.0 g of the reactant to 0.2 g is :

An increase in the concentration of the reactants of a reaction leads to change in :

For the chemical reaction
N2(g) + 3H2(g) ⇌ 2NH3(g)
the correct option is :

If the rate constant for a first order reaction is k, the time (t) required for the completion of 99 % of the
reaction is given by :

When initial concentration of the reactant is
doubled, the half-life period of a zero order
reaction

The correct difference between first and
second order reactions is that

Mechanism of a hypothetical reaction
X2 + Y2 \(\to\) 2XY, is given below :
(i)   X2 \(\to\) X + X (fast)
(ii)  X + Y2 \(\rightleftharpoons\) XY + Y (slow)
(iii) X + Y \(\to\) XY (fast)
The overall order of the reaction will be

A first order reaction has a specific reaction rate of 10\(-\)2 sec\(-\)1. How much time will it take for 20 g of the reactant to reduce to 5 g?

The decomposition of phosphine (PH3) on tungsten at low pressure is a first-order reaction. It is because the

The addition of a catalyst during a chemical reaction alters which of the following quantities?

The rate of first-order reaction is 0.04 mol L\(-\)1 s\(-\)1 at 10 seconds and 0.03 mol L\(-\)1 s\(-\)1 at 20 seconds after initiation of the reaction. The half-life period of the reaction is

The activation energy of a reaction can be determined from the slope of which of the following graphs?

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is

The rate constant of the reaction A \(\to\) B is 0.6 \(\times\) 10\(-\)3 mol L\(-\)1 s\(-\)1. If the concentration of A is 5 M, then concentration of B after 20 minutes is

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. The order of reaction is

For a reaction between A and B the order with respect to A is 2 and the other with respect to B is 3. The concentrations of both A and B are doubled, the rate will increase by a factor of

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20oC to 35oC?
(R = 8.314 J mol\(-\)1 K\(-\)1)

In a zero-order reaction, for every 10oC rise of temperature, the rate is doubled. If the temperature is increased from 10oC to 100oC, the rate of the reaction will become

In a reaction, A + B \(\to\) product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentration of both the reactants (A and B) are doubled, rate law for the reaction can be written...

Activation energy (E\(a\)) and rate constants (k1 and k2) of a chemical reaction at two different temperatures (T1 and T2) are related by

Which one of the following statements for the order of a reaction is incorrect?

The rate of the reaction :   2N2O5 \(\to\) 4NO2 + O2
can be written in three ways.
\({{ - d\left[ {{N_2}{O_5}} \right]} \over {dt}} = k\left[ {{N_2}{O_5}} \right]\)
$${{d\left[ {N{O_2}} \right]} \over {dt}} = k'\left[ {{N_2}{O_5}} \right...

The unit of rate constant for a zero order reaction is

The half-life of a substance in a certain enzyme-catalysed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg L\(-\)1 to 0.04 mg L\(-\)1 is

During the kinetic study of the reaction, 2A + B \(\to\) C + D, following results were obtained

.tg {border-collapse:collapse;border-spacing:0;}
.tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;bor...

For the reaction N2O5(g) \(\to\)  2NO2(g) + 1/2O2(g) the value of rate of disappearance of N2O5 is given as 6.25 \(\times\) 10\(-\)3 mol L\(-\)1 s\(-\)1. The rate of formation of NO2 and O2 is given respectively as

The rate of the reaction, 2NO + Cl2 \(\to\) 2NOCl is given by the rate equation rate = k[NO]2[Cl2]. The value of the rate constant can be increased by

Half-life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is