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Published on: 27/08/2019
Chemical Kinetics
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Questions + Answers key
Take MCQ Chemistry Test
1.
Identify the reaction order from each of the following rate constants.
(i) k = 2.3 \(\times\) 10-5 L mol -1 s-1
(ii) k = 3 10-4 \(\times\) s -1
2.
For a zero order reaction will the molecularity be equal to zero?
3.
For a reaction A + B \(\to\) Products, the rate law is Rate = k[A] [B]3/2. Can the reaction be an elementary reaction?
4.
State a condition in which bimolecular reaction is kinetically first order reaction.
5.
Express the relation between the half-life period of a reactant and its initial concentration for a reaction of nth order.
6.
Is there any reaction for which reaction rate does not decrease with them?
7.
The rate of reaction X \(\to\) Y becomes 8 times when the concentration of the reactant X is doubled. Write the rate law of the reaction.
8.
Express the rate of the following reaction in terms of disappearance of hydrogen in the reaction: 3H2 (g) + N2 (g) \(\to\) 2 NH3 (g).
9.
For the reaction Cl2(g) + 2NO(g) \(\to\) 2NOCl(g) the rate law is expressed as rate = k[Cl2][NO]2 What is the overall order of this reaction?
10.
Why does the rate of a reaction not remain constant throughout the reaction process?
11.
Rate constant of a reaction (k) is 175 litre2 mol-2 sec-1. What is the order of reaction?
first
second
third
zero
12.
A first order reaction has a half-life period of 34.65 seconds. Its rate constant is
2 \(\times 10\) -2 sec-1
4 \(\times 10\) -4 sec-1
20 sec-1
2 \(\times 10\) -4 sec-1
13.
The unit of rate constant for a zero order reaction is
mol L-1 s-1
L mol-1 s-1
L2mol-1 s-1
s-1
14.
The rate of the reaction 2 NO + CI2 \(\rightarrow\) 2NOCI is given by the rate equation : rate = k [NO]2 [CI2]. The value of the rate constant can be increased by
increasing the temperature
increasing the concentration of NO
increasing the concentration of CI2
doing all of these
15.
In the reaction BrO-3 (aq) + 5 Br - (aq) + 6 H+ \(\longrightarrow\) 3 Br2(I) + 3 H2O (l), the rate of apperance of bromine (BHr2) is related to the disapearance of bromide uions as follows :
\(\frac { d[{ Br }_{ 2 }] }{ dt } =-\frac { 5 }{ 3 } \frac { d[{ Br }^{ - }] }{ dt } \)
\(\frac { d[{ Br }_{ 2 }] }{ dt } =\frac { 5 }{ 3 } \frac { d[{ Br }^{ - }] }{ dt } \)
\(\frac { d[{ Br }_{ 2 }] }{ dt } =\frac {3 }{ 5} \frac { d[{ Br }^{ - }] }{ dt } \)
\(\frac { d[{ Br }_{ 2 }] }{ dt } =-\frac { 3 }{ 5 } \frac { d[{ Br }^{ - }] }{ dt } \)
16.
Zero order reactions
17.
COCI2 \(\longrightarrow\) CO + CI2
18.
2 H2O2 \(\longrightarrow\) 2H2O + O2
19.
2 NH3 \(\longrightarrow\) N2 + 3 H2
20.
2 HI \(\longrightarrow\) H2 + I2
1.
(i) The unit of second order rate constant is L mol–1 s–1, therefore k = 2.3 x 10–5 L mol–1 s–1 represents a second order reaction.
(ii) The unit of a first order rate constant is s–1 therefore k = 3 x 10–4 s–1 represents a first order reaction.
2.
No, molecularity can never be equal to zero or in fraction.
3.
No, it is not elementary reaction. Had this be elementary reaction order with respect to 'B' should have been 1.
4.
When one of the reactants is in excess, bimolecular reaction becomes kinetically first order.
5.
\(t_{1 / 2} \propto \frac{1}{[R]_0^{n-1}}\) where 'n' is order of reaction.
6.
Yes, zero order reaction.
7.
\(\frac{d x}{d t}=\mathrm{k}[\mathrm{X}]^3 \text { as } 2^3=8 \ \therefore \text { order is } 3 .\)
8.
\(-\frac{1}{3} \frac{d\left[H_2\right]}{3 d t}\) represents rate of reaction.
9.
The overall order of reaction is 3.
10.
It is because concentration of reactants goes on decreasing with time.
11.
(c) : On the basis of given units of k, the reactions of 3 rd order.
12.
(a) : \(k = \frac {0.693}{t/2}= \frac {0.693}{34.65}s^{-1} = 2 \times 10^{-2}\)s-1
13.
(a) Rate = \(\frac {dx}{dt} = k[A_o]^{o} = k \) or \(k = \frac {dx}{dt} = \frac {conc}{Time} =\frac {mol L^{-1}}{s}\)mol L-1 s-1.
14.
(a) : The rate of constant of a reaction depends only on temperature and does not depend upon concentrations of the reactants.
15.
(d) \(\frac{1}{3} \frac { d[{ Br }_{ 2 }] }{ dt } =-\frac { 1 }{ 5 } \frac { d[{ Br }^{ - }] }{ dt } \) or \(\frac { d[{ Br }_{ 2 }] }{ dt } =-\frac {3 }{ 5 } \frac { d[{ Br }^{ - }] }{ dt } \)
16.
( )
t 100% = [A]0/k
17.
( )
1\(\frac {1}{2}\)
18.
( )
1
19.
( )
0
20.
( )
2
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