NEET Chemistry Chapter Wise Mock Test – Chemical Kinetics

NEET Chemistry Chapter Wise Mock Test – Chemical Kinetics

Question 1:
For the reaction, 2A + B—> Products; the active mass of B is kept constant, and that of A is doubled. The rate of reaction will be then
(a) decrease 4 times
(b) decrease 2 times
(c) increase 4 times
(d) increase 2 times

Question 2:

Question 3:

Question 4:

Question 5:
A drop of solution (volume = 0.05 mL) contains 60.0x 10^-7 molof H⁺ . If the rate of disappearance of H+ is 6.0x 10⁵mol/Ls, how long will it take  for H⁺ to disappear fro the drop?
(a) 8.0 x 10^-8s
(b) 2.0 x 10^-8s
(c) 6×10^-6
(d) 2.0 x 10^-2s

Question 6:

Question 7:

Question 8:

Question 9:

Question 10:

Question 11:
if a certain reaction is first order with respect to A, second order with respect to B and zero order with respect to C then what is the order of reaction?
(a) First
(b) Second
(c) Third
(d) Zero

Question 12:
For a reaction between A and B, the initial rate of reaction is measured for various initial concentrations of A and B. The data provided areThe overall order of the reaction is
(a) one
(b) two
(c) two and half
(d) three

Question 13:
The rate constant of a zero order reaction is 0.2 mol dm^-3 h^-1 . If the concentration of the reactant after 30 min is 0.05 mol dm-3. Then, its initial concentration would be,
(a) 0.01 mol dm^-3
(b) 0.15 mol dm^-3
(c) 0.25 mol dm^-3
(d) 4.00mol dm^-3

Question 14:
The half-life period for zero order reaction A-—> Product; is 100 min. How long will it take in 80% completion?
(a) 80 min
(b) 160 min
(c) 100 min
(d) 200 min

Question 15:

Question 16:
For a reaction aA —» x P, when [A] = 2.2 mM, the rate was found to be 2.4 m Ms^-1. On reducing concentration of A to half, the rate changes to 0.6 m Ms^-1. The order of reaction with respect to A is
(a) 1.5
(b) 2.0
(c) 2.5
(d) 3.0

Question 17:
In the reaction, 2N₂0₅—> 4N0₂ + 0₂ , initial pressure is 500 atm and rate constant k is 3.38 x 10^-5s^-1. After 10 min, the final pressure of N₂0₅ is
(a) 490 atm
(b) 250 atm
(c) 480 atm
(d) 420 atm

Question 18:

Question 19:
A first order reaction is 50% completed in 1.26 x 10¹⁴ s. How much time would it take for 100% completion?
(a) 1.26 x 10¹⁵s
(b) 2.52 x 10¹⁴s
(c) 2.52 x 10²⁵s
(d) Infinite

Question 20:
The value of rate constant of a pseudo first order reaction
(a) depends on the concentration of reactants present in small amount
(b) depends on the concentration of reactants present in excess
(c) is independent of the concentration of reactants
(d) depends only on temperature

Question 21:
For a first order reaction, the concentration changes s; from 0.8 to 0.4 in 15 min. The time taken for the $ concentration to change from 0.1 M to 0.025 M is it
(a) 30 min
(b) 15 min
(c) 7.5 min
(d) 60 min

Question 22:
t_1/4 can be taken as the time taken for the concentration of a reactant to drop to 3/4 th of its initial value. If the rate constant for a first order reaction is k, the t_1/4 can be Witten as
(a) 0.75Ik
(b) 0.69Ik
(c) 0.29Ik
(d) 0.101k

Question 23:
A first order reaction is 75% complete after 32 min. When was 50% of the reaction completed?
(a) 16 min
(b) 8 min
(c) 4 min
(d) 32 min

Question 24:
The concentration of reactant X decreases from 0.1 M to 0,005 M in 40 min. If the reaction follows first order kinetics, the rate of reaction when concentration of X is 0.01 M will be
(a) 1.73x 10^-4 M mint^-1
b ) 3.47 x 10^-4 M min^-1
(c) 3.47 x 10^-5 M min^-1
(d) 7.50 xIO^-4 min^-1

Question 25:
Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law, with f1/2=3.00h. What fraction of sample of sucrose remains after 8 h?
(a) 1.023 M
(b) 0.8725 M
(c) 0.023 M
(d) 0.1576 M

Question 26:
The rate of first order reaction is 1.5x 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 27:
For a first order reaction, A >B, the reaction rate at reactant concentration of 0.01 M is found to be 2.Ox 10^-5 mol L^-1 s^-1. The half-life period of the reaction is ,
(a) 220 s
(b) 30 s
(c) 300 s
(d) 347 s

Question 28:
The half-life of the reaction; ‘N₂₀5 > 2N0+1/20₂; is 2.4 h. Starting with 10.8 g of N₂O₅ , how much oxygen will be obtained after period of 9.6 h?
(a) 1.5 L
(b) 3.36 L
(c) 1.05 L
(d) 0.07 L

Question 29:
After how many seconds will the concentration of the reactant in a first order reaction be halved if tHevrate constant is 1.155 x 10^-3 s^-1?
(a) 600
(b) 100
(c) 60
(d) 10

Question 30:
The ratio of the times of 99.9% of the reaction to complete and half of the reaction to complete is .,.
(a) 2
(b) 4
(c) 8
(d) 10

Question 31:
The activation energy of a reaction is 9 kcal/mol. The . increase in the rate constant when its temperature is raised from 295 to 300 K is approximately
(a) 10%
(b) 50%
(c) 100%
(d) 29%

Question 32:
The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy (Ea) of the reaction?
(a) 1842.4 R
(b) 921.2 R
(c) 460.6 R
(d) 230.3 R

Question 33:
Activation energy of a chemical reaction can be determined by
(a) evaluating rate constant at standard temperatures
(b) evaluating velocities of reaction at two different temperatures
(c) evaluating rate constant at two different temperatures
(d) changing concentration of reactants .

Question 34:
The temperature coefficient of most of the reactions lies between
(a) 1 and 3
(b) 2 and 3
(c) 1 and 4
(d) 2 and 4

Question 35:
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 36:

Question 37:
The rate constant is doubled when temperature increases from 27° C to 37° C. Activation energy in kJ is
(a) 34
(b) 54
(c) 100
(d) 53

Question 38:
Which of the following statements 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) I and II
(c) II and III
(d) All of these

Question 39:
In the presence of a catalyst, activation energy of a reaction lowered by 2 kcal at 27°C. Hence, rate will be
(a) 20 times
(b) 28 times
(c) 14 times
(d) remain the same

Question 40:
When we increase temperature, the rate of reaction increase because of
(a) more number of collisions
(b) decrease in mean free path
(c) more number of energetic collisions
(d) less number of energetic collisions

Question 41:
Pick the appropriate choice about collision theory of reaction rates.
I. It explains the effect of temperature on rate of reaction
II. It assumes that the reactants must be in correct orientate to react.
III. It says rate depends upon the frequency at which reactants collide.
IV. The collisions having energy higher than the threshold value will give successful reactions.
The correct points are
(a) I, III and IV
(b) II and IV
(c) I and IV
(d) I. II, III and IV

Direction (Q. Nos. 42-43) In the following questions, more than one of the answers given may be correct. Select the correct answer and mark it according to the codes.
Codes
(a) 1,2 and 3 are correct
(b) 1 and 2 are correct
(c) 2 and 4 are correct
(d) 1 and 3 are correct

Question 42:
Select the correct statements with respect of zero order reaction.
1. The rate of the reaction is independent of temperature.
2. The rate of the reaction is independent of reactant concentration.
3. The rate constant of the reaction is independent of temperature.
4. The rate constant of the reaction is independent of reactant concentration.

Question 43:
For the first order reaction,
1. the degree of dissociation is equal to (1 – e^-ktw).
2. a plot of reciprocal concentration of the reactant versus times gives a straight line.
3. the pre-exponential factor in the Arrhenius equation has the dimension of time, t^-1.
4. the time taken for the completion of 75% reaction is thrice the 1/2 of the reaction

Question 44:

Question 45:

Direction (Q. NOS. 46-48) Each of these questions contains two statements: Assertion and Reason. Each of these questions also has four alternative choices, only one of which is the correct answer. You have to select one of the codes (a), (b), (c) and (d) given below.
(a) Assertion is true, Reason is true; Reason is the correct explanation of the Assertion
(b) Assertion is true, Reason is true; Reason is not the correct explanation of the Assertion
(c) Assertion is true, Reason is false .
(d) Assertion is false, Reason is true

Question 46:
Assertion The order of a reaction can have fractional -value.
Reason The order of a reaction cannot be written from balanced equation of a reaction.

Question 47:
Assertion Molecularity has no meaning for a complex reaction.
Reason The overall molecularity of a complex reaction is equal to the molecularity of the slowest step.

Question 48:

Question 49:

Question 50:
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) zero
(b) first
(c) second
(d) more than zero but less than first

Question 51:
What is the activation energy for a reaction if its rate doubles when temperature is raised from 20°C to 35°C? (R = 8.314 J^-1 K^-1)
(a) 269 kJ mol^-1
(b) 34.7 kJ mol^-1
(d) 15.1 kJ mol^-1
(d) 342 kJ mol^-1

Question 52:
A reaction having equal energies of activation for forward and reverse reaction has
(a) ΔG = 0
(b) Δ H= 0
(C)ΔH = ΔG=ΔS=0
(d) Δ S = 0

Question 53:
In a zero order reaction for every 10° 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 54:
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 concentrations 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 55:
2N₂0₅ (g) —> 4N0₂ (g) + 02(g) What is the ratio of the rate of rate of formation of N0₂?
(a) 1 : 2
(b) 2 : 1
(c) 1 : 4
(d) 4 : 1

Question 56:
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) -1
(b) -2
(c) 1
(d) 2

Question 57:
For a first order reaction A—> B, the reaction rate at reactant concentration of 0.01 M is found to be 2.0x 10^-5 mol L^-1 s^-1. The half-life period of the reaction is
(a) 220 s
(b) 30  s
(c) 300 s
(d) 347 s

Question 58:
Which one of the following statements for the order of a reaction is incorrect?
(a) Order is not influenced by stoichiometric coefficient of the reactants
(b) Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction
(c) Order of reaction is always whole number
(d) Order can be determined only experimentally

Question 59:
Half-life of a reaction is found to be inversely proportional to the cube of initial concentration. The order of reaction is
(a) 5
(b) 2
(c) 4
(d) 3

Question 60:
A schematic plot of In K_eq versus inverse of temperature for a reaction is shown below:

The reaction must be
(a) highly spontaneous at ordinary temperature
(b) one with negligible enthalpy change
(c) endothermic
(d) exothermic

Question 61:
At a certain temperature, the first order rate constant, k₁ is found to be smaller than the second order rate constant, k₂. If the energy of activation, E, of the first order reaction is greater than energy of activation, E₂ of the second order reaction then with increase in temperature
(a) will increase faster than k₂, but always will remain less than k₂
(b) k₂ will increase faster than f₁,
(c) k₁, will increase faster than k₂ and becomes equal to k₂
(d) k₁, will increase faster than k₂ and becomes greater than k₂

Answers:

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