MDCAT XI Chemistry Chemical Kinetics Online Test-2

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Created on July 10, 2025 By

old.medicoengineer.com

MDCAT XI Chemistry Chemical Kinetics Online Test-2

📚 Test Details

Subject: Chemistry
Class: 1st year / XI
Chapter: Chemical Kinetics
Test: 2
Book: Sindh Textbook
Total No. Of MCQs: 50 MCQs
Time Allowed: 50 Minutes
Price: Free

NameEmailPhone Number

1 / 50

1. The rate of a chemical reaction tells us about:

a) the reactants taking part in the reaction

b) the products formed in the reaction

c) how slow or fast the reaction is taking place

d) none of the above

2 / 50

2. Which of the following observations is incorrect about the order of a reaction?

a) Order of a reaction is always a whole number

b) The stoichiometric coefficient of the reactants doesn’t affect the order

c) Order of reaction is the sum of powers to express the rate of reaction in terms of the concentration of reactants

d) Order can only be assessed experimentally

3 / 50

3. The rate constant of a zero-order reaction has the unit:

a) s⁻¹

b) mol L⁻¹ s⁻¹

c) L² mol⁻² s⁻¹

d) L mol⁻¹ s⁻¹

4 / 50

4. For the reaction:
2A + B → A₂B
If the concentration of A is doubled and that of B is halved, then the rate of the reaction will:

a) increase 2 times

b) increase 4 times

c) decrease 2 times

d) remain the same

5 / 50

5. When the rate of the reaction is equal to the rate constant, the order of the reaction is:

a) zero order

b) first order

c) second order

d) third order

6 / 50

6. In the Haber process for the manufacture of ammonia, the following catalyst is used:

a) Platinized asbestos

b) Iron

c) Copper oxide

d) Alumina

7 / 50

7. A catalyst alters which of the following in a chemical reaction?

a) Entropy

b) Enthalpy

c) Internal energy

d) Activation energy

8 / 50

8. The reaction NO₂ + CO → NO + CO₂ takes place in two steps. Find the rate law:
Step 1: 2NO₂ → NO + NO₃ (k₁) – slow
Step 2: NO₃ + CO → CO₂ + NO₂ (k₂) – fast

a) R = k₁ [NO₂]³

b) R = k₂ [NO₃] [CO]

c) R = k₁ [NO₂]

d) R = k₁ [NO₂]²

9 / 50

9. Hassan performs the reaction:
X + H₂O → product.
Find the rate of reaction if the value of X is 2 M and k is 4.

a) 8

b) 16

c) 4

d) 2

10 / 50

10. What is the rate law for the acid hydrolysis of an ester such as CH₃COOC₂H₅ in aqueous solution?

a) k [CH₃COOC₂H₅]

b) k [CH₃COOC₂H₅] [H₂O]

c) k [CH₃COOC₂H₅]²

d) k

11 / 50

11. When light strikes on Cs metal and it ejects electrons to become positively charged, the order of its reaction is:

a) 1st order

b) 2nd order

c) 3rd order

d) Zero order

12 / 50

12. Catalyst which enhances reactant activity used in the decomposition of H₂O₂ to H₂ and I₂:

a) Glycerine

b) Fe

c) V₂O₅

d) None of these

13 / 50

13. Mazhar performs an experiment on a reaction in which H₂O reacts with H₂O and ionization occurs. The order of the reaction is:

a) Pseudo zero order

b) Zero order

c) Pseudo first order

d) Second order

14 / 50

14. Thermo-decomposition of N₂O₅ is:
2N₂O₅(g) ⟶ 2N₂O₄(g) + O₂(g)

a) Zero order

b) 1st order

c) 3rd order

d) 2nd order

15 / 50

15. With an increase of 10°C, the rate of reaction doubles. This increase in the rate of reaction is due to:

a) Decrease in activation energy of reaction

b) Decrease in the number of collisions between reactant molecules

c) Increase in activation energy of reactants

d) Increase in number of effective collisions

16 / 50

16. The reaction: 2A + B ⟶ C + D
The expression for the rate law is: rate = k [A]⁰ [B]
The order of reaction in A is:

a) First

b) Second

c) Third

d) Zero

17 / 50

17. The rate of an enzyme-catalyzed reaction is independent of:

a) Concentration of substrate

b) Concentration of product

c) Enzyme

d) Temperature

18 / 50

18. Reactions with high activation energy are usually:

a) Fast

b) Slow

c) Exothermic

d) Reversible

19 / 50

19. If CaCO₃ breaks into CaO and CO₂, and for supposition its activation energy is low, it means:

a) Rate of forward and backward is fast

b) Rate of backward is fast only

c) Rate of forward is fast only

d) Rate of forward and backward is slow

20 / 50

20. Activated complex:

a) Unstable high energy

b) Unstable lower energy

c) Stable at higher energy

d) Stable lower energy

21 / 50

21. Which of the following is an example of homogeneous catalysis?

a) Hydrolysis of ester

b) Oxidation of ammonia to NO

c) Hydrogenation of unsaturated hydrocarbons

d) Conversion of SO₂ to SO₃ in contact process

22 / 50

22. A catalyst does not change the:

a) Activation energy

b) Path

c) Total amount

d) All are changed by catalyst

23 / 50

23. Order of reaction is strictly determined by the:

a) Stoichiometry of the balanced equation

b) Experiment

c) Total number of molecules participating in the reaction

d) Fast step of reaction mechanism

24 / 50

24. If X and Y are the enzymes performing reactions, the reactions will be ______ by enzymes:

a) Exothermic

b) Endothermic

c) Both of these

d) None of these

25 / 50

25. Radioactivity of a radioactive metal is termed as:

a) 1st order

b) 2nd order

c) 3rd order

d) Zero order

26 / 50

26. Rate = k[A]²[B]

a) Value of k increases 4 times when concentration of A becomes double

b) Value of k decreases 2 times when concentration of B becomes half

c) Value of k remains unchanged by decreasing or increasing concentration of A or B

d) None of these

27 / 50

27. The rate of reaction increases with temperature due to:

a) Decrease in activation energy

b) Increase in activation energy

c) Increase in frequency of collision

d) Increase in concentration

28 / 50

28. When the rate of reaction is equal to the rate constant, the order of reaction is:

a) 3

b) 0

c) 1

d) 2

29 / 50

29. If the temperature is decreased from 100°C to 80°C, then the rate of reaction:

a) Increases 4 times

b) Increases 8 times

c) Increases 2 times

d) None of these

30 / 50

30. Oxidation of chloroform to phosgene gas:

a) Iron powder is a positive catalyst.

b) V₂O₅ is a positive catalyst

c) 2% ethanol is a negative catalyst

d) Glycerine is a negative catalyst.

32 / 50

32. The decomposition of H₂O₂ is decreased by:

a) 2% ethanol

b) Glycerine

c) MnO₂

d) V₂O₅

33 / 50

33. In the reaction X ⟶ Y, the rate of appearance is written as:

a) –dX/dt

b) –dY/dt

c) +dY/dt

d) None of these

34 / 50

34. A reaction proceeds in such a way that the order of reaction is independent of reactant concentration. The overall order of the reaction would be:

a) First

b) Second

c) Third

d) Zero

35 / 50

35. The unit of k is mol dm⁻³ s⁻¹. The order of reaction is:

a) 0

b) 1

c) 2

d) 3

36 / 50

36. The rate constant k of a reaction is affected by:

a) Concentration of reactant

b) Concentration of product

c) Pressure

d) Temperature

37 / 50

37. Which of the following is an example of acid catalysis?

a) Hydrolysis of ester

b) Decomposition of H₂O₂

c) Oxidation of chloroform

d) Auto-oxidation of KMnO₄ and oxalic acid

38 / 50

38. Initial rate of reaction is slow; as soon as the product is formed, the rate of reaction increases.

a) Homogeneous catalysis

b) Heterogeneous catalysis

c) Auto catalysis

d) Inhibitor

39 / 50

39. For a fast reaction:

a) Activation energy is low and rate constant is low

b) Activation energy is high and rate constant is high

c) Activation energy is high and rate constant is low

d) Activation energy is low and rate constant is high

40 / 50

40. Which of the following factors affects the rate of a chemical reaction?

a) Temperature

b) Concentration of reactants

c) Presence of a catalyst

d) All of the above

41 / 50

41. What is the study of reaction rates and reaction mechanisms called?

a) Thermodynamics

b) Chemical kinetics

c) Stoichiometry

d) Thermochemistry

42 / 50

42. Which of the following is NOT a factor that affects reaction rate?

a) Molecularity

b) Temperature

c) Catalyst

d) Concentration

43 / 50

43. For a zero-order reaction, the rate of reaction is:

a) Dependent on the concentration of reactants.

b) Independent of the concentration of reactants

c) Directly proportional to the concentration of reactants

d) Inversely proportional to the concentration of reactants

44 / 50

44. Rate of reaction generally:

a) Increases gradually

b) Decreases instantaneously

c) Increases at end

d) Decreases gradually

45 / 50

45. Greater the concentration of reactant, __________.

a) Greater will be dX/dt

b) Lesser will be dX/dt

c) dX/dt will be moderate

d) Any of the above

46 / 50

46. Activated complex is formed due to:

a) Pressure

b) Effective collision

c) Ineffective collisions

d) Temperature

47 / 50

47. Rate of reaction when the concentrations of reactants are taken as unity is called:

a) Arrhenius constant

b) Molecularity

c) Specific rate constant

d) Ideal rate constant

48 / 50

48. Sum of exponents of molar concentrations is called:

a) Order of reaction

b) Molecularity

c) Rate of reaction

d) Average of reaction

49 / 50

49. Energy of activation for the backward reaction is less than the forward reaction for a __________ reaction.

a) Endothermic

b) Exothermic

c) Moderate

d) Fast

50 / 50

50. When the reaction completes in more than one step, the rate of reaction will be determined by:

a) Fast step

b) Slowest step

c) All steps

d) Molecularity of the reaction

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MDCAT XI Chemistry Chemical Kinetics Online Test-2

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