Chemical Kinetics Test

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Chemical Kinetics Test - 10

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Question 1
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Direction (Q. Nos. 1-13) This section contains multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct
Q. In the following reaction, which has maximum rate w.r.t. rate of disappearance of NH₃?
4NH₃ + 50₂→ 4NO + 6H₂O

A
O₂

B
NO

C
H₂O

D
Equal

Solution

By stoichiometry of the reaction
Question 2
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The rate of formation of NO(g) in the reaction, 2NOBr(g) → 2NO(g) + Br₂(g) was reported as 1.6 x 10^-4 Ms^-1. Thus, rate of the reaction is

A
1.6 x 10^-4Ms^-1

B
8.0 x 10^-5MS^-1

C
3.2 x 10^-4Ms^-1

D
6.4 x 10^-4MS^-1

Solution
Question 3
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Rate of formation of SO₃ in the reaction below is 100 kg min^-1.
2SO₂+ O₂ → 2SO₃
Hence, rate of disappearance of SO₂ will be:

A
100kg min^-1

B
80 kg min^-1

C
64 kg min^-1

D
32 kg min^-1

Solution

Rate of disappearance of SO₂ = Rate of formation of SO₃ But quantity is to be expressed in terms of moles.
Rate of formation of SO₃ = 100 kg SO₃ min-¹
Question 4
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The following reaction can take place in both directions:

For the forward reaction, the rate varies with the concentration of A as and for the backward reaction,

Hence, net reaction rate is:

A
= K₁[A] - K₂[B]

B
= (K_{1 -}K₂[B])

C
= (K₁[A]-K₂)

D
= (k₁-k₂)

Solution
Question 5
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For a reaction, xA → yB, rate of disappearance of ‘A’ is related to the rate of appearance of 'B' by the equation
Thus, x and y respectively are

A
1,2

B
2,4

C
1/2, 2

D
4,1

Solution
Question 6
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For the reaction,
H₂(g) + A₂(g) 2H(g) + A₂(g)
k_f = 2.2 x 10⁴ L mol^-1s^-1 and K_c = 1.00 x 10^-4 at 3000 K. Thus, k_b is

A
2.2 x 10⁸ L²mol^-2s^-1

B
0.45 x 10^-8L^-2mol²s^-1

C
2.2 L mol^-1s^-1

D
0.45L^-1mol s^-1

Solution
Question 7
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For a reaction,

hen x, y and z are

A
1:1:1

B
3:2:3

C
3:3:2

D
2:2:3

Solution

For the reaction: xA + yB → zC

Given that,

Multiplying equation 2 by 1/3, we get

On comparing equation 1 and 3,
x = 3, y = 3, z = 2.
Question 8
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For the reaction,
2N₂O₅(g) → 4NO₂ (g) + O₂(G)
Thus,

A
k₁ = k₂= k₃

B
2k₁ = k₂= 4k₃

C
2k₁ = 4k₂= k₃

D
None of these

Solution
Question 9
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The decomposition of acetaldehyde is given by the following reaction:
CH₃CHO(g) → CH₄(g) + CO(g)
Rate of the reaction with respect to the pressure of the reactant is

A
- dp/dt

B

C

D
none

Solution
Question 10
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For the reaction,
then rate law is

A

B

C

D

Solution
Question 11
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For gaseous reaction, the rate can be expressed as

A

B

C

D
none of these

Solution
Question 12
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The initial rates of reaction for the equation, 2A + B → Products.
Products were determined under various initial concentrations of reactants.
Thus, rate law is equal to

A
k[A][B]

B
k[A][B]²

C
k[A]

D
k[B]

Solution

Let order w.r.t. A = a, order w.r.t. B = b
Question 13
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For the reaction, A + 2B → Product, the reaction rate was halved on doubling the concentration of A. Thus, order w.r.t. A is

A
1

B
1/2

C
-1/2

D
-1

Solution

If concentration of the nth order reaction is made m time, rate becomes mⁿ times.
Question 14
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Direction (Q. Nos. 14 and 15) This section contains a passage describing theory, experiments, data, etc. Two questions related to the paragraph have been given. Each question has only one correct answer out of the given 4 options (a), (b), (c) and (d)
Passage
The decomposition of NO₂ at 400 K proceeds at a of rate of 5.4 x 10^-5 mol L^-1 s^-1 when [NO₂] = 0.01 mol^-1
2 NO₂(g) → 2NO(g ) + O₂(g).
Q. What is the rate law when observed rate is 1.35 x 10^-5 mol L^-1 s^-1at [NO₂] = 0.005 mol L^-1?

A
k[NO₂]

B
k[NO₂]²

C
k[NO₂]³

D
k[NO₂]⁰

Solution

Given unit of rate = mol L^-1 s^-1
General formula for unit of rate = mol ^n-1 L^n-1 s ^-1
On equating,
1-n = 1 ⇒ n = 0
n-1 = -1 ⇒ n = 0
Hence, it is a zero order reaction.
Question 15
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The decomposition of NO₂ at 400 K proceeds at a of rate of 5.4 x 10^-5 mol L^-1 s^-1 when [NO₂] = 0.01 mol^-1
2 NO₂(g) → 2NO(g ) + O₂(g).
Q. Rate constant of the reaction will be

A
0.54 L mol^-1 s^-1

B
0.54 x 10^-3 L mol^-1 s^-1

C
5.4 s^-1

D
0.54s^-1

Solution
Question 16
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Direction (Q. Nos. 16-18) This section contains 3 questions. When worked out will result in one integer from 0 to 9 (both inclusive)
In the following reaction
Q. Where negative sign indicates rate of disappearance of the reactant. What is the value of x/y ?

A
2

B
4

C
5

D
6

Solution
Question 17
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The reaction rate is defined as the rate at which the concentration of the reactants __________ with time or the concentration of products ___________ with time.

A
Increase, increase

B
Decrease, decrease

C
Decrease, increase

D
Increase, decrease

Solution

The reaction rate is defined as the rate at which the concentration of the reactants decreases with time or the concentration of products increases with time.
Question 18
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In a certain polluted atmosphere containing O₃ at a steady concentration of 2.0 x 10^-6 M, the hourly production of O₃ by all sources was estimated as 7.2 x 10^-15 M. If the only mechanism for destruction of O₃ in the second-order reaction is
2O₃ → 3O₂
then rate constant for destruction reaction, defined by the rate law for - Δ[O₃]/Δf is x * 10^-7 M^-1 s^-1 . What is the value of x?

A
5

B
2

C
7

D
8

Solution
Question 19
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Only One Option Correct Type
This section contains 2 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct
For a reversible reaction, net rate is
hence given reaction is

A

B

C

D
None of these

Solution

2A - B →(reversible) C
For a forward reaction, (dx/dt)_f = k₁[A]² [B]^-1
For a backward reaction, (dx/dt)_b = k₂[C]
Net rate = (dx/dt)_f - (dx/dt)_b= k₁[A]₂ [B]^-1 - k₂[C]
Question 20
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Reaction kinetics deals with the study of

A
Rate of reaction

B
Mechanism of reaction

C
Factors which affects the rate of reaction

D
All of the mentioned

Solution

Reaction kinetics deals with the study of rate of reaction, their mechanism and the factors which affects the rate of reaction. It specifies all the general characteristics of a chemical reaction.