Chemical Kinetics Test

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Chemical Kinetics Test - 4

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Question 1
1 / -0

Study of rate of chemical reaction is known as

A
Chemical change

B
Chemical equilibrium

C
Chemical thermodynamics

D
Chemical kinetics

Solution

Chemical kinetics is the branch of chemistry which deals with the study of rate of reaction, factors affecting the rate of reaction and mechanism of the chemical reaction.
Question 2
1 / -0

For which of the following reaction the units of rate constant and rate of the reaction are same?

A
Third order reaction

B
Zero order reaction

C
First order reaction

D
Second order reaction

Solution

Rate = k[Reactant]⁰
Question 3
1 / -0

R₁ is the rate of a simple reaction 2NO + O₂ 2NO₂.
If the volume of the reaction vessel is doubled, the rate of the reaction becomes

A
1/8 R₁

B
8 R₁

C
R₁

D
1/2 R₁
Question 4
1 / -0

The rate of reaction can be measured as

A
Rate of reaction can be measured in terms of Rate of disappearance of reactant or rate of appearance of product

B
Rate of appearance of the product

C
Rate of appearance of reactant

D
Rate of disappearance of reactant

Solution

rate of reaction = (+) rate of appearance of products = (-) rate of disappearance of reactants
Question 5
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The inversion of cane sugar is represented by C₁₂H₂₂O₁₁ + H₂O C₆H₁₂O₆ + C₆H₁₂O₆. This reaction is a

A
second-order reaction

B
unimolecular reaction

C
pseudo-unimolecular reaction

D
None of these
Question 6
1 / -0

Which among the following is an instantaneous reaction?

A
Precipitation of silver chloride.

B
Burning of a log of wood

C
Rusting of iron

D
Hydrolysis of starch

Solution

Mixing of silver nitrate and sodium chloride involves ionic reaction to form precipitates of silver chloride.
AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)
Since ionic reactions are very fast, so it is an instantaneous reaction.
Question 7
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Directions: The following question has four choices out of which ONLY ONE is correct.

Which of the following statements is not true in terms of reaction kinetics?

A
A catalyst speeds up a reaction by lowering the activation energy.

B
Rise of temperature increases the rate as the number of molecules increases.

C
Increase of concentration speeds up a reaction as it increases the collision frequency.

D
Removal of product from the reaction vessel as soon as it is formed increases the reaction rate as it increases the collision frequency of reactant molecules.
Question 8
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For the reaction 2A 3B, the rate of reaction may be represented as

A
r = – d[A]/dt = d[B]/dt

B
r = – d[A]/dt = (1/3) d[B]/dt

C
r = – (1/2) d[A]/dt = (1/3) d[B]/dt

D
r = (1/2) d[A]/dt = – (1/3) d[B]/dt
Question 9
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A catalyst is a substance which

A
increases the equilibrium concentrations of the products

B
decreases the energy of activation

C
does not alter reaction mechanism

D
increases the frequency of collision of reacting species
Question 10
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The half-life of a second-order reaction A B is given as

A
t_1/2 = 0.693/k

B
t_1/2 = k/[A₀]

C
t_1/2 = [A]₀/k

D
t_1/2 = 1/k[A]₀
Question 11
1 / -0

The rate constant, the activation energy and the Arrhenius parameter of a chemical reaction at 50^oC are 7.3 10⁴ s^-¹, 18.23 KJ mol^-1 and 6.0 10⁴ s^-1, respectively. The value of the rate constant as T approaches is

A
6.479 10⁷ s^-1

B
8.22 10¹ s^-1

C
8.105 10²³ s^-1

D
infinity
Question 12
1 / -0

In a chemical reaction, if a linear (y = mx) graph is obtained between half-life and concentration of reactants, then what is the order of the reaction?

A
0

B
1

C
3

D
2
Question 13
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The units of rate of reaction and its rate constant

A
are identical

B
are quite independent of each other

C
depend on the experimental conditions of the reaction

D
are related to each other through a definite expression depending upon the order of the reaction
Question 14
1 / -0

_{The half-life of a zero-order reaction A}_{B is}

A
directly proportional to the concentration of A

B
independent of the concentration of A

C
inversely proportional to the concentration of A

D
determined by the concentration of B
Question 15
1 / -0

The reaction 2N₂O₅ (g) 4 NO₂(g) + O₂(g) provides a linear plot when ln is plotted against t with a negative slope. The decomposition of N₂O₅ follows

A
zero-order kinetics

B
first-order kinetics

C
third-order kinetics

D
second-order kinetics

Question 16

1 / -0

Match the following:

Column – I	Column – II
(A) Zero-order reaction	(a) High activation energy
(B) Pseudo unimolecular reaction	(b) Decreases activation energy
(C) Slow reaction	(c) Decomposition of ammonia on tungsten
(D) Positive catalyst	(d) Hydrolysis of cane sugar

(A) – (c), (B) – (d), (C) – (a), (D) – (b)

(A) – (d), (B) – (a), (C) – (c), (D) – (b)

(A) – (c), (B) – (b), (C) – (a), (D) – (d)

(A) – (a), (B) – (d), (C) – (c), (D) – (b)

Question 17
1 / -0

The temperature coefficient of a reaction is

A
the rate constant at a fixed temperature

B
the ratio of the rate constants at two different temperatures

C
the ratio of the rate constants at temperatures differing by at least 25^oC

D
the ratio of the rate constants at temperatures differing by 10^oC (say from 25^oC to 35^oC)
Question 18
1 / -0

The activation energy in a chemical reaction is defined as

A
the difference in energies of reactants and products

B
the sum of energies of reactants and products

C
the difference in energies of intermediate complexes with the average energy of reactants and products

D
the difference in energies of intermediate complexes and the average energy of reactants
Question 19
1 / -0

Molecularity of a reaction

A
Cannot be less than 2

B
Can be zero

C
Is always a whole number

D
Can have a fractional values

Solution

Molecularity means minimum no. of atoms molecules or ions which undergo collision for conversion of reactant to Product. So it is a whole no. Cannot be fractional or negative.
Question 20
1 / -0

On increasing the pressure three folds, the rate of reaction, 2H₂S + O₂ products, would increase by how many times?

A
3 times

B
9 times

C
12 times

D
27 times
Question 21
1 / -0

The rate constant of reaction A → 2B is 1.0 × 10^-3 mol L^-1 min^-1. If the initial concentration of A is 1.0 mol L^-1, then what is the concentration of B after 100 minutes?

A
0.1 mol L^-1

B
0.2 mol L^-1

C
0.9 mol L^-1

D
1.8 mol L^-1
Question 22
1 / -0

For a first-order reaction, the ratio of times to complete 99.9% and half of the reaction is

A
8

B
9

C
10

D
12
Question 23
1 / -0

For a first-order reaction,

A
the degree of dissociation of reactants is equal to 1 – exp (– kt)

B
the pre-exponential factor in the Arrhenius equation has the dimension of time

C
the time taken for the completion of 75% reaction is thrice of half-life time

D
a plot of reciprocal of concentration of the reactant versus time is a straight line
Question 24
1 / -0

If the initial concentration of a reactant of a zero order reaction is reduced by half, the time for half decomposition

A
remains the same

B
increases to twice its original value

C
decreases to half its original value

D
increases to four times its original value
Question 25
1 / -0

A catalyst is added to a reaction to increase the rate of reaction. Which of the following statements is correct?

A
A catalyst increases the activation energy between reactants and products and hence, lowers the potential energy barrier.

B
A catalyst provides an alternate pathway or reaction mechanism.

C
A catalyst alters G, Gibbs energy of reaction.

D
A catalyst changes the equilibrium constant of a reaction.

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Chemical Kinetics Test - 4

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Chemical Kinetics Test - 4

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Question 1

Chemical change

Chemical equilibrium

Chemical thermodynamics

Chemical kinetics

Solution

Question 2

Third order reaction

Zero order reaction

First order reaction

Second order reaction

Solution

Question 3

1/8 R1

8 R1

R1

1/2 R1

Question 4

Rate of reaction can be measured in terms of Rate of disappearance of reactant or rate of appearance of product

Rate of appearance of the product

Rate of appearance of reactant

Rate of disappearance of reactant

Solution

Question 5

second-order reaction

unimolecular reaction

pseudo-unimolecular reaction

None of these

Question 6

Precipitation of silver chloride.

Burning of a log of wood

Rusting of iron

Hydrolysis of starch

Solution

Question 7

A catalyst speeds up a reaction by lowering the activation energy.

Rise of temperature increases the rate as the number of molecules increases.

Increase of concentration speeds up a reaction as it increases the collision frequency.

Removal of product from the reaction vessel as soon as it is formed increases the reaction rate as it increases the collision frequency of reactant molecules.

Question 8

r = – d[A]/dt = d[B]/dt

r = – d[A]/dt = (1/3) d[B]/dt

r = – (1/2) d[A]/dt = (1/3) d[B]/dt

r = (1/2) d[A]/dt = – (1/3) d[B]/dt

Question 9

increases the equilibrium concentrations of the products

decreases the energy of activation

does not alter reaction mechanism

increases the frequency of collision of reacting species

Question 10

t1/2 = 0.693/k

t1/2 = k/[A0]

t1/2 = [A]0/k

t1/2 = 1/k[A]0

Question 11

6.479 107 s-1

8.22 101 s-1

8.105 1023 s-1

infinity

Question 12

0

1

3

2

Question 13

are identical

are quite independent of each other

depend on the experimental conditions of the reaction

are related to each other through a definite expression depending upon the order of the reaction

Question 14

directly proportional to the concentration of A

independent of the concentration of A

1/8 R₁

8 R₁

R₁

1/2 R₁

t_1/2 = 0.693/k

t_1/2 = k/[A₀]

t_1/2 = [A]₀/k

t_1/2 = 1/k[A]₀

6.479 10⁷ s^-1

8.22 10¹ s^-1

8.105 10²³ s^-1

the ratio of the rate constants at temperatures differing by at least 25^oC

the ratio of the rate constants at temperatures differing by 10^oC (say from 25^oC to 35^oC)

0.1 mol L^-1

0.2 mol L^-1

0.9 mol L^-1

1.8 mol L^-1