XI Chemistry Chemical Kinetics Online Test Mdcat-2024

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Test Details:

Subject: Chemistry
Class: 1st year or 11
Chapter name: Chemical Kinetics
Test: MDCAT 2024
Book: Sindh Textbook
Total No. Of MCQS: 50
Time Allowed: 50 Minutes
Price : Free

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Created on July 21, 2024 By

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XI Chemistry Chemical Kinetics Online Test Mdcat-2024

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1 / 51

1. Chemical Kinetics can be defined as:

a) The study of the energy changes during chemical reactions.

b) The study of the rates of chemical reactions and the factors affecting them.

c) The study of the equilibrium positions of chemical reactions.

d) The study of the formation and properties of chemical bonds.

2 / 51

2. What is the unit of the rate of a chemical reaction?

a) Molarity (M)

b) Moles per liter (mol/L)

c) Moles per liter per second (mol/L·s)

d) Liters per second (L/s)

3 / 51

3. What does the rate law of a reaction express?

a) The equilibrium constant of the reaction.

b) The relationship between the reaction rate and the concentration of reactants.

c) The enthalpy change of the reaction.

d) The volume change during the reaction

4 / 51

4. In the rate law Rate = k[A][B], if the concentration of A is doubled and the concentration of B is halved, how does the rate change?

a) The rate remains unchanged

b) The rate increases by a factor of 2

c) The rate decreases by a factor of 2

d) The rate increases by a factor of 4

5 / 51

5. What does the term "reaction order" refer to in a rate law?

a) The total number of molecules in the reaction

b) The ratio of reactants to products.

c) The sum of the exponents in the rate law expression.

d) The time it takes for the reaction to complete.

6 / 51

6. The rate constant of a reaction is found to be 0.05 L·mol־¹·s־¹. What is the reaction order?

a) Zero-order

b) First-order

c) Second-order

d) Third-order

7 / 51

7. If the rate of a reaction is given by Rate = k[A][B]², how does the rate change if [A] is increased by a factor of 3 and [B] is increased by a factor of 2?

a) The rate increases by a factor of 6.

b) The rate increases by a factor of 12.

c) The rate increases by a factor of 18.

d) The rate increases by a factor of 36.

8 / 51

8. Which of the following statements is true about the rate constant (k) in the rate law expression?

a) The rate constant depends on the concentration of reactants.

b) The rate constant is constant and does not change with temperature.

c) The rate constant changes with temperature.

d) The rate constant is always equal to 1.

9 / 51

9. What is the order of a reaction if the rate law is given by Rate = k[A][B]²?

a) Zero-order

b) First-order

c) Second-order

d) Third-order

10 / 51

10. Unit of rate constant for zero order reaction is same as

a) Unit of first order reaction

b) Unit of Second Order reaction

c) Unit of rate of reaction

d) None

11 / 51

11. Unit of rate constant for first order reaction is

a) mol/dm³.s

b) dm³/mol

c) s־¹

d) All

12 / 51

12. Photoelectric effect is a

a) First order reaction

b) Second Order Reaction

c) Third order reaction

d) Zero order reaction

13 / 51

13. Rate determining step can be observed in

a) Elemantary reactions

b) Complex reactions

c) One step reactions

d) None

14 / 51

14. In a reaction between Nitrogen dioxide and Carbon monoxide, following statements cannot be true

a) It is a bimolecular reaction

b) It is a second order reaction with respect to Carbon monoxide

c) reaction rate will increase 4 times if concentration of NO₂ is doubled

d) None as all are correct

15 / 51

15. Rate of reaction is affected by nature of reactants because of their

a) Structure

b) Nature of bonding

c) Physical state

d) all of these

16 / 51

16. How does the bond strength of reactants affect the rate of a reaction?

a) Weaker bonds generally lead to faster reactions

b) Stronger bonds generally lead to faster reactions.

c) Bond strength has no effect on the rate of reaction.

d) Bond strength only affects the equilibrium position.

17 / 51

17. How does increasing the concentration of a reactant generally affect the rate of a chemical reaction?

a) The rate decreases.

b) The rate remains unchanged

c) The rate increases.

d) The rate first increases and then decreases.

18 / 51

18. For a reaction where the rate law is Rate = k[A]², if the concentration of A is tripled, by what factor does the rate of reaction change?

a) The rate increases by a factor of 3.

b) The rate increases by a factor of 6.

c) The rate increases by a factor of 9.

d) The rate decreases by a factor of 3.

19 / 51

19. In a first-order reaction, what happens to the rate of reaction if the concentration of the reactant is doubled?

a) The rate decreases by half.

b) The rate remains unchanged.

c) The rate doubles.

d) The rate increases by a factor of four.

20 / 51

20. If the concentration of all reactants in a reaction is doubled, and the reaction rate increases by a factor of 8, what is the order of the reaction with respect to the reactants?

a) First-order

b) Second-order

c) Third-order

d) Fourth-order

21 / 51

21. Which factor does NOT affect the rate of a chemical reaction?

a) Concentration of reactants

b) Temperature

c) Nature of the reactants

d) Color of the reactants

22 / 51

22. How does increasing the temperature generally affect the rate of a reaction?

a) The rate decreases.

b) The rate remains unchanged.

c) The rate increases.

d) The rate first increases and then decreases

23 / 51

23. Which of the following statements is true about the effect of surface area on the rate of a reaction?

a) Increasing the surface area of a solid reactant decreases the reaction rate.

b) Increasing the surface area of a solid reactant has no effect on the reaction rate

c) Increasing the surface area of a solid reactant increases the reaction rate

d) The surface area of a liquid reactant affects the reaction rate.

24 / 51

24. Increase in temperature increases the reaction rates of all:

a) Exothermic reaction

b) Endothermic reaction

c) Both of them

d) None

25 / 51

25. With the increase of 10°C temperature the rate of reaction doubles.This increase in 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

d) Increase in number of effective collision

26 / 51

26. The experimental relationship between a reaction rate and the concentration of the reactants is called

a) Order law

b) Rate law

c) Molecularity

d) Order of reaction

27 / 51

27. For a reaction

H₂(g) + Br₂(g) -----> 2HBr(g)

The experimental data suggests Rate = K [H₂][Br₂]½.

What will be the order of reaction?

a) 1

b) 3/2

c) 0.5

d) 2

28 / 51

28. According to collision theory, which of the following conditions must be met for a reaction to occur?

a) Reactant molecules must collide with sufficient energy.

b) Reactant molecules must collide with correct orientation.

c) Reactant molecules must collide with sufficient energy and correct orientation.

d) Reactant molecules must have a low activation energy.

29 / 51

29. What is the transition state in a chemical reaction?

a) The reactants before they collide.

b) The products after the reaction has occurred.

c) A high-energy intermediate state during the reaction.

d) The state where reactants and products are in equilibrium

30 / 51

30. Which of the following statements best describes activation energy?

a) The energy required to form the products from the reactants.

b) The energy released during the formation of the transition state.

c) The minimum amount of energy that reactant molecules need to undergo a chemical reaction.

d) The energy difference between the reactants and the products.

31 / 51

31. Which type of catalyst is involved in the same phase as the reactants?

a) Homogeneous catalyst

b) Heterogeneous catalyst

c) Enzyme catalyst

d) Photocatalyst

32 / 51

32. Catalyst used in oxidation of Chloroform is _____ and it's nature is___

a) Glycerin ,Positive

b) Glycerin, Negative

c) 2%ethyl alcohol, Positive

d) 2% ethyl alcohol, Negative

33 / 51

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

a) The decomposition of hydrogen peroxide using manganese dioxide

b) The hydrolysis of ester using sulphuric acid to produce acetic acid and alcohol

c) The hydrogenation of alkenes using a platinum catalyst

d) The decomposition of ozone using chlorine radicals

34 / 51

34. A reaction involving two different reactants can never be:

a) Unimolecular reaction

b) First order reaction

c) Second-order reaction

d) Bimolecular reaction

35 / 51

35. At low temperature, the reaction, CO(g) + NO2(g) = CO2(g) + NO(s) is zero order in CO and second order in NO2. The rate law is, rate =

a) k[CO][NO2]

b) k[NO2]

c) k[CO]²[NO2]

d) k[NO2]²

36 / 51

36. The rate of reaction when the concentration of reactants are takes as unity is called

a) Equilibrium constant

b) specific rate constant

c) Arrhenius constant

d) Plank’s constant

37 / 51

37. All of the following statements about type of catalysis are correct EXCEPT:

a) Homogeneous Catalysis – Catalyst and reactants are in the same phase.

b) Heterogeneous catalysis – catalyst and reactants are not in the same phase

c) Many heterogeneous have catalyst in the solid state that catalyze reactants in the gaseous states

d) In heterogeneous catalysis, the reaction takes place at the surface of solid and absorption of

38 / 51

38. How does a negative catalyst affect a chemical reaction?

a) It increases the activation energy.

b) It decreases the activation energy.

c) It remains unchanged.

d) It does not participate in the reaction

39 / 51

39. In the decomposition of hydrogen peroxide, which substance can act as a negative catalyst to slow down the reaction?

a) Glycerine

b) Sodium hydroxide (NaOH)

c) Manganese dioxide (MnO₂)

d) Potassium iodide (KI)

40 / 51

40. In the Haber’s process for the formation of NH3, why Fe catalyst is finely divided:

a) to reduce surface area

b) to reduce its loss during the reaction

c) To produce the maximum reduction in the Ea

d) to increase surface area

41 / 51

41. Which of the following does not influence the rate of a reaction?

a) Nature of reactants

b) Temperature of reaction

c) Concentration of reactants

d) Molecularity of reaction

42 / 51

42. In some reactions a product formed acts as a catalyst. This phenomenon is called

a) Negative catalysis

b) Heterogeneous catalysis

c) Activation of catalyst

d) Autocatalysis

43 / 51

43. For the reaction 4A + B------> 2C + 2D, which of the following statements is not correct?

a) Rate of disappearance of B is 1/4 the of rate of disappearance of A

b) Rate of formation of C is 1/2 the rate of consumption of A

c) Rate of appearance of D is 1/2 the rate of disappearance of B

d) Rate of formation of C and d are equal C

44 / 51

44. In the fermentation of sugarcane into commercial alcohol which enzymes are used

a) Sucrase and Invertase

b) Zymase and Invertase

c) Amylase and Zymase

d) Protease and Lipase

45 / 51

45. Negative catalyst are also called as

a) Inhibitor

b) Retarding catalyst

c) Autocatalyst

d) Both A and B

46 / 51

46. Which of the following best defines heterogeneous catalysis?

a) Catalysis where the reactants and the catalyst are in the same phase.

b) Catalysis where the reactants and the catalyst are in different phases.

c) Catalysis where the catalyst is consumed during the reaction.

d) Catalysis that occurs without any catalyst.

47 / 51

47. Examples of zero order reaction

a) Reaction of H₂ and Cl₂

b) Photosynthesis

c) Photography

d) All of these

48 / 51

48. Ionic reactions are classified into

a) Slow reactions

b) Fast reactions

c) Moderate reactions

d) Reversible reactions

49 / 51

49. The best alternative tern for the velocity of the reaction is

a) Rate of appearance

b) Rate of disappearance

c) Average rate

d) Instantaneous rate

50 / 51

50. In a multi step reaction the rate determining step is always

a) The first step

b) The last step

c) The slow step

d) The fast step

51 / 51

51. A substance which increase the rate of reaction without being consumed during the reaction is called

a) An autocatalyst

b) A catalyst

c) A negative catalyst

d) All of these

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