MCQ Question for Class 12 Chemistry Chapter 4 Chemical Kinetics

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Chemical Kinetics Class 12 MCQ Questions with Answers

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Question. The decomposition of phosphine (PH₃) on tungsten at low pressure is a first-order reaction. It is because the
(a) rate is proportional to the surface coverage
(b) rate is inversely proportional to the surface coverage
(c) rate is independent of the surface coverage
(d) rate of decomposition is very slow.

Question. The rate constant of the reaction A B is 0.6 × 10^–3 mol L–1 s^–1. If the concentration of A is 5 M, then concentration of B after 20 minutes is
(a) 3.60 M
(b) 0.36 M
(c) 0.72 M
(d) 1.08 M 

Question. For a reaction between A and B the order with respect to A is 2 and the order with respect to B is 3.
The concentrations of both A and B are doubled, the rate will increase by a factor of
(a) 12
(b) 16
(c) 32
(d) 10

Question. In a reaction, A + B → 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 as
(a) rate = k[A][B]²
(b) rate = k[A]²[B]²
(c) rate = k[A][B]
(d) rate = k[A]²[B]

Question. Which one of the following statements for the order of a reaction is incorrect?
(a) Order can be determined only experimentally.
(b) Order is not influenced by stoichiometric coefficient of the reactants.
(c) Order of a reaction is sum of power to the concentration terms of reactants to express the rate of reaction.
(d) Order of reaction is always whole number.

Question. The unit of rate constant for a zero order reaction is
(a) mol L^–1 s^–1
(b) L mol^–1 s^–1
(c) L2 mol^–2 s^–1
(d) s^–1

Question. For the reaction, A + B → products, it is observed that
(i) on doubling the initial concentration of A only, the rate of reaction is also doubled and
(ii) on doubling the initial concentration of both A and B, there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is given by
(a) rate = k[A][B]²
(b) rate = k[A]²[B]²
(c) rate = k[A][B]
(d) rate = k[A]²[B]

Question. 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
(a) 2
(b) –2
(c) 1
(d) –1

Question. If the rate of the reaction is equal to the rate constant, the order of the reaction is
(a) 0
(b) 1
(c) 2
(d) 3 

Question. 2A B → C, It would be a zero order reaction when
(a) the rate of reaction is proportional to square of concentration of A
(b) the rate of reaction remains same at any concentration of A
(c) the rate remains unchanged at any concentration of B and C
(d) the rate of reaction doubles if concentration of B is increased to double.

Question. For the reaction; 2N₂O₅ → 4NO₂ + O₂ rate and rate constant are 1.02 × 10^–4 and 3.4 × 10^–5 sec–1 respectively, then concentration of N₂O₅ at that time will be
(a) 1.732
(b) 3
(c) 1.02 × 10^–4
(d) 3.4 × 10₅

Question. The given reaction,
2FeCl₃ + SnCl₂ → 2FeCl₂ + SnCl₄ is an example of
(a) third order reaction
(b) first order reaction
(c) second order reaction
(d) none of these.

Question. The rate constant for a first order reaction is 4.606 × 10^–3 s^–1. The time required to reduce 2.0 g of the reactant to 0.2 g is
(a) 100 s
(b) 200 s
(c) 500 s
(d) 1000 s 

Question. 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
(a) t = 2.303/k
(b) t = 0.693/k
(c) t = 6.909/k
(d) t = 4.606/k

Question. A first order reaction has a rate constant of 2.303 × 10^–3 s^–1. The time required for 40 g of this reactant to reduce to 10 g will be [Given that log₁₀ 2 = 0.3010]
(a) 230.3 s
(b) 301 s
(c) 2000 s
(d) 602 s

Question. The correct difference between first and second order reactions is that
(a) the rate of a first-order reaction does not depend on reactant concentrations; the rate of a second-order reaction does depend on reactant concentrations
(b) the half-life of a first-order reaction does not depend on [A]0 ; the half-life of a second-order reaction does depend on [A]0
(c) a first-order reaction can be catalysed; a secondorder reaction cannot be catalysed
(d) the rate of a first-order reaction does depend on reactant concentrations; the rate of a secondorder reaction does not depend on reactant concentrations. 

Question. When initial concentration of the reactant is doubled, the half-life period of a zero order reaction
(a) is halved
(b) is doubled
(c) is tripled
(d) remains unchanged.

Question. 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?
(a) 138.6 sec
(b) 346.5 sec
(c) 693.0 sec
(d) 238.6 sec 

Question. 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
(a) 44.1 s
(b) 54.1 s
(c) 24.1 s
(d) 34.1 s

Question. When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is
(a) second
(b) more than zero but less than first
(c) zero
(d) first. 

Question. A reaction is 50% complete in 2 hours and 75% complete in 4 hours. The order of reaction is
(a) 1
(b) 2
(c) 3
(d) 0

Question. The half-life of a substance in a certain enzymecatalysed 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
(a) 414 s
(b) 552 s
(c) 690 s
(d) 276 s 

Question. Half-life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is
(a) 0.5 × 10–2 s^–1
(b) 0.5 × 10–3 s^–1
(c) 5.0 × 10–2 s^–1
(d) 5.0 × 10–3 s^–1 

Question. If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately (log 4 = 0.60,log 5 = 0.69)
(a) 45 minutes
(b) 60 minutes
(c) 40 minutes
(d) 50 minutes.

Question. For a first order reaction A B the reaction rate at reactant concentration of 0.01 M is found to be 2.0 × 10^–5 mol L–1 s^–1. The half-life period of the reaction is
(a) 30 s
(b) 220 s
(c) 300 s
(d) 347 s 

Question. The rate of a first order reaction is 1.5 × 10^–2 mol L^–1 min^–1 at 0.5 M concentration of the reactant. The half-life of the reaction is
(a) 0.383 min
(b) 23.1 min
(c) 8.73 min
(d) 7.53 min

Question. The reaction 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 ?
(a) 1 hour
(b) 0.5 hour
(c) 0.25 hour
(d) 2 hours

Question. Raw milk sours in about 4 hat 27°C, but in about 48 h in a refrigerator at 17°C. What is the activation energy for souring of milk?
(a) 78.0 kl mol^-1
(b) 46.21 kl mol^-1
(c) 23.5 kl mol^-1
(d) 80.8 kl mol^-1

Question. A plot of 1/ T versus k for a reaction gives the slope – 1 x 10⁴ K. The energy of activation for the reaction is (Given, R = 8.314K^-1 mol^-1)
(a) 83.14 J mol^-1
(b) 1.202 kJ mol^-1
(c) 12.02 J mol^-1
(d) 83.14 kJ mo1^-1

Question. The rate constant (k₁ ) of one of the reaction is found to be double that of the rate constant (k₂ ) of another reaction. The relationship between the corresponding activation energies of the two reactions E_a1 and E_a2 will be
(a) E_a1 < E_a2
(b) E_a1 > E_a2
(c) E_a1 = E_a2
(d) E_a1 = 2E_a2

Question. For a reaction taking place in three steps, the rate constants are k₁ , k₂ and k₃ and overall rate constant is k = k₁k₃ / k₂ . If the energies of activation E₁, E₂ and E₃ are 60, 30 and 10 kJ mol^-1 , respectively, then the overall energy of activation is
(a) 30 kJ mol^-1
(b) 40 kJ mol^-1
(c) 60 kJ mol^-1
(d) l00 kJ mol^-1

Question. The rate ofreaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be(R = 8.314 JK^-1 mol^-1 and log 2 = 0.301)
(a) 53.6 kJ mol^-1
(b) 48.6 kJ mol^-1
(c) 58.5 kJ mol^-1
(d) 60.5 kJ mol^-1

Question. A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be k₁ and k₂ respectively. Then
(a) k₂ ≈ 0.25 k₁
(b) k₂ ≈0.5 k₁
(c) k_{2 ≈} 4 k₁
(d) k₂ ≈ 2 k₁

Question. The rate of a reaction is doubled for every 10° rise in temperature. The increase in reaction rate as a result of temperature rise from 10° to 100° is
(a) 112
(b) 512
(c) 400
(d) 614
(e) 100

Question. N₂ (g) + 2H₂ (g) ⇌ 2NH₃ (g) + 22 kcal
The activation energy for the forward reaction is 50 kcal. What is the activation energy for the backward reaction?
(a) 72 kcal
(c) -72 kcal
(b) 28 kcal
(d) -28kcal

Question. A given sample of milk turns sour at room temperature (27°C) in 5 h. In a refrigerator at -3° C., it can be stored 10 times longer. The energy of activation for the souring of milk is
(a) 2.303 x 5 R kJ mol^-1
(b) 2.303 x 3 R kJ mol^-1
(c) 2.303 x 2.7 R kJ mol^-1
(d) 2.303 x 10 R kl mol^-1

Question. The rate of a chemical reaction doubles for every 10°C rise of temperature. If the temperature is raised by 50°C., the rate of the reaction increases by about
(a) IO times
(b) 24 times
(c) 32 times
(d) 64 times

Question. A reactant ( A ) forms two products

Question. The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol^-1. The ratio of rate constant to the Arrhenius factor is
(a) 0.01
(b) 0.1
(c) 0.02
(d) 0.001

Question. The activation energy of exothermic reaction A ➔ B 80 kJ mol^-1. The heat of reaction is 200 kJ mol^-1. The activation energy for the reaction B ➔ A (in kJ mol^-1) will be
(a) 80
(b) 120
(c) 40
(d) 280

Question. In the given graph the activation energy, E_a for the reverse reaction will be 

(a) 50 kJ
(b) 50 kJ
(c) 200 kJ
(d) 100 kJ

Question. By increase in temperature by 10 K, the rate of reaction becomes double. How many times the rate of reaction will be if the temperature is increased from 303K to 353 K?
(a) 4
(b) 8
(c) 16
(d) 32

Question. Plots showing the variation of the rate constant ( k) with temperature (T) are given below. The plot that follows Arrhenius equation is

Question. For a first order reaction A ➔ P, the temperature (T) dependent rate constant ( k) was found to follow the equation log k = – (2000)/ T + 6.0 The pre-exponential factor A and the actjvation energy Ea, respectively, are
(a) 1.0 x 10⁶s^-1 and 9.2 kJ mol^-1
(b) 6.0s^-1 and 16.6 kJ mol^-1
(c) 1.0 x 10⁶s^-1 and 16.6 kJ mol^-1
(d) 1.0 x 10⁶s^-1 and 38.3 kJ mol^-1

Question. The activation energies of two reactions are E₁ and E₂ (E₁ > E ). If the temperature of the system is increased from T₁ to T₂ , the rate constant of the reactions changes from k₁ to k₂ in the first reaction and k₂ to k₂ in the second reaction. Preruct which of the following expression is correct ?
(a) k₁ / k₁ = k₂ / k₂
(b) k₁ / k₁ > k₂ / k₂
(c) k₁ / k₁ < k₂ / k₂
(d) k₁ / k₁ = k₂ / k₂ = 1
(e) k₁ / k₁ = k₂ / k₂ = 0

Question. Which of the following statement is in accordance with collision theory ?
I. Rate is directly proportional to collision frequency
II. Rate depends upon orientation of atoms
III. Temperature determines the rate
(a) Only III
(b) Only I and II
(c) Only II and III
(d) All of these

Question. If k₁ = rate constant at temperature T₁ and k₂ = rate constant at temperature T₂ for a first order reaction, then which of the following relations is correct?
(Ea : activation energy)

Question. For a reversible reaction, A ⇌ B,
which one of the following statements is wrong from the given energy profile diagram ?

(a) Activation energy of forward reaction is greater than backward reaction
(b) The forward reaction is endothermic
(c) The threshold energy is less than that of activation energy
(d) The energy of activation of forward reaction is equal to the sum of heat of reaction and the energy of activation of backward reaction

Question. If Xis the total number of collisions which a gas molecule register with others per unit time under particular conditions, then the collision frequency of the gas containing N molecules per unit volume is 
(a) X / N
(b) NX
(c) 2 NX
(d) NX / 2

Question. For a first-order reaction, the half-life period is independent of
(a) first power of final concentration
(b) cube root of initial concentration
(c) initial concentration
(d) square root of final concentration.

Question. For a reaction, activation energy Ea = 0 and the rate constant at 200 K is 1.6 × 10⁶ s^–1. The rate constant at 400 K will be [Given that gas constant R = 8.314 J K^–1 mol^–1]
(a) 3.2 × 104 s^–1
(b) 1.6 × 106 s^–1
(c) 1.6 × 103 s^–1
(d) 3.2 × 106 s^–1

Question. The addition of a catalyst during a chemical reaction alters which of the following quantities?
(a) Enthalpy
(b) Activation energy
(c) Entropy
(d) Internal energy

Question. What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20 °C to 35 °C? (R = 8.314 J mol^–1 K^–1)
(a) 34.7 kJ mol^–1
(b) 15.1 kJ mol^–1
(c) 342 kJ mol^–1
(d) 269 kJ mol^–1

Question. In a zero-order reaction, for every 10 °C rise of temperature, the rate is doubled. If the temperature is increased from 10 °C to 100 °C, the rate of the reaction will become
(a) 256 times
(b) 512 times
(c) 64 times
(d) 128 times.

Question. The rate of the reaction,
2NO + Cl₂ → 2NOCl is given by the rate equation, rate = k[NO]₂[Cl₂]. The value of the rate constant can be increased by
(a) increasing the temperature
(b) increasing the concentration of NO
(c) increasing the concentration of the Cl₂
(d) doing all of these.

Question. The activation energy for a simple chemical reaction A ⇌ B is Ea in forward direction. The activation energy for reverse reaction
(a) is negative of Ea
(b) is always less than Ea
(c) can be less than or more than Ea
(d) is always double of Ea. 

Question. When a biochemical reaction is carried out in laboratory, outside the human body in absence of enzyme, then rate of reaction obtained is 10^–6 times, the activation energy of reaction in the presence of enzyme is
(a) 6/RT
(b) P is required
(c) different from Ea obtained in laboratory
(d) can’t say anything. 

Question. How enzymes increases the rate of reactions?
(a) By lowering activation energy
(b) By increasing activation energy
(c) By changing equilibrium constant
(d) By forming enzyme substrate complex

Question. Activation energy of a chemical reaction can be determined by
(a) evaluating rate constants at two different temperatures
(b) evaluating velocities of reaction at two different temperatures
(c) evaluating rate constant at standard temperature
(d) changing concentration of reactants. 

Question. By the action of enzymes, the rate of biochemical reaction
(a) does not change
(b) increases
(c) decreases
(d) either (a) or (c).

Question. An increase in the concentration of the reactants of a reaction leads to change in
(a) activation energy
(b) heat of reaction
(c) threshold energy
(d) collision frequency.

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