List of top Chemistry Questions on Chemical Kinetics asked in NEET (UG)

A first order reaction has a specific reaction rate of 10^–2 s^–1. How much time will it take for 20 g of the reactant to reduce to 5 g?

Mechanism of a hypothetical reaction \(X_2 + Y_2→ 2XY\) is given below :
(i) \(X_2→ X + X\) (fast)
(ii) \(X + Y_2⇋ XY + Y\) (slow)
(iii) \(X + Y → XY\) (fast)
The overall order of the reaction will be

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

The rate of a 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 rate constant of the reaction $ A \to B$ is $0.6 \times 10^{-3}$ mole per second. If the concentration of A is 5 M, then concentration of $B$ after 20 minutes is :

In a reaction, A + B $\rightarrow$ Product, rate is doubled when the concentration of B is doubled and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled. Rate law for the reaction can be written as

The rate of the reaction $ {2 N_2 O_5 -> 4 NO_2 + O_2}$ can be written in three ways: $\frac{-d [N_2 O_5]}{dt} = k [N_2 O_5]$ $\frac{d[NO_2]}{dt} = k' [N_2 O_5]$ $\frac{d[O_2]}{dt} = k" [N_2 O_5]$ The relationship between k and k' and between k and k'' are-

During the kinetic study of the reaction, $2A + B\longrightarrow C + D$, following results were obtained . Based on the above data which one of the following is correct?

Run	$A/mol\,L^{-1}$	$B/mol\,L^{-1}$	Initial rate of formation of $D/mol\,L^{-1}\,min^{-1}$
I	0.1	0.1	$6.0 \times 10^{-3}$
II	0.3	0.2	$7.2 \times 10^{-2}$
III	0.3	0.4	$2.88 \times 10^{-1}$
IV	0.4	0.1	$2.40 \times 10^{-2}$

The rate of the reaction $ {2NO + Cl_2 -> 2NOCl}$ is given by the rate equation rate = $ { k[NO]^2[Cl_2]}$ . The value of the rate constant can be increased by -

In the reaction $BrO _{3}^{-}( aq )+5 Br ^{-}( aq )+6 H ^{+} \rightarrow 3 Br _{2}(l)+3 H _{2} O (l)$ The rate of appearance of bromine $\left( Br _{2}\right)$ is related to rate of disappearance of bromide ions as following

For the reaction, $N _{2}+3 H _{2} \rightarrow 2 NH _{3}$, If $\frac{ d \left[ NH _{3}\right]}{ dt }=2 \times 10^{-4}\, mol\, L ^{-1} s ^{-1}$, The value of $\frac{- d \left[ H _{2}\right]}{ dt }$ would be -

Half-life period of a first order reaction is $1386\, s.$ The specific rate constant of the reaction is

The rate constants $k_1$ and $k_2$ for two different reactions are $10^{16} .e^{-2000/T}$ and $10^{15} .e^{-1000/T}$,respectively. The temperature at which $k_1= k_2$ is

If $60\%$ of a first order reaction was completed in $60\, min$, $50\%$ of the same reaction would be completed in approximately ($log\, 4 = 0.60 \,log\, 5 = 0.69$)

The reaction of hydrogen an iodine monochloride is given as $H _{2( g )}+2 ICl _{( g )} \rightarrow 2 HCl _{( g )}+ I _{2( g )}$ This reaction is of first order with respect to $H _{2( g )}$ and $ICl _{( g )}$, following mechanisms were proposed Mechanism $A$: $H _{2( g )}+2 ICl _{( g )} \rightarrow 2 HCl _{( g )}+ I _{2( g )}$ Mechanism $B$ : $H _{2( g )}+ ICl _{( g )} \rightarrow HCl _{( g )}+ HI _{( g )} ;$ Slow $HI _{( g )}+ ICl _{( g )} \rightarrow HCl _{( g )}+ I _{2( g )} ;$ Fast Which of the above mechanism $(s)$ can be consistent with the given information about the reaction:

Consider the reaction, $N_2(g)+3H_2(g) \to 2NH_3(g)$ The equality relationship between $\frac{d[NH_3]}{dt}$ and $-\frac{d [H_2]}{dt}$ is :-

For a first order reaction, $A \longrightarrow B$, the reaction rate at reactant concentration of $0.01\, M$ is found to be $2.0 \times 10^{-5} \, mol \, \, L^{-1} s^{-1}$. The half-life period of the reaction is

The rate of reaction between two reactants A and B decreases by a factor of 4,if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is:

The rate of first order reaction is $1.5 \times 10^{-2}$ mol $L^{-1} \, min^{-1}$ at 0.5 M concentration of the reactant. The half-life of the reaction is

The activation energy for a simple chemical reaction, $A\longrightarrow$ B is $E_{a}$ in forward direction. The activation energy for reverse reaction

If the rate of a reaction is equal to the rate constant, the order of the reaction is

The reaction \(\text {A→B}\) follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B.

The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, $k = A.e ^{- E ^{*} / RT }$. Activation energy $\left( E ^{*}\right)$ of the reaction can be calculated by plotting

2A \(\rightarrow\) B + C
It would be a zero-order reaction when