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Are you preparing for your upcoming CBT exams and want a solid way to test your knowledge and build confidence? We’ve got something exciting for you—CBT Practice Questions with a built-in timer to simulate real exam pressure and boost your speed.

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There are 40 questions which you are to answer in 15 minutes that gives you roughly 30 seconds per question.

If you can get at least 60%, you can be rest assured that you’ll ace CHM 101 exam

In a normal exam you will be asked between 40 – 60 questions but I only arranged 40 questions

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Move as fast as possible and starting with questions that don’t have calculation first to save time

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Created on April 24, 2025 By

Phil

EBSU CHM 101

1 / 50

1. Water is an example of

A. Compound

B. An ion

C. An element

D. A mixture

2 / 50

2. Which of the following supports Boyles law

A. K=PV

B. T = KV

C. NRT=KV

D. PV/R

3 / 50

3. The sum of all exponents of the reactants as contained in the experimentally determined rate law is known as

A. Overall rate law

B. Overall equilibrium law

C. Overall molecularity of reaction

D. Overall order of reaction

4 / 50

4. The factor 0.001 corresponds to which prefix

A. Centi

B. Milli

C. deka

D. Deci

5 / 50

5. An expression which shows how a reaction is related to concentration is termed

A. Equilibrium Law

B. Molecularity of reaction

C. Rate Equation

D. Order of reaction

6 / 50

6. Calculate the percentage composition of Nitrogen in Magnesium Nitrate Mg(No3)2

Mg =24.31

N= 14.01

O= 16

A. 0.01889%

B. 0.1889%

C. 1.889%

D. 18.99%

7 / 50

7. Rate of a reaction is measured in

A. 𝑚𝑜𝑙 𝑐𝑚−1𝑠𝑒𝑐−3

B. 𝑚𝑜𝑙 𝑐𝑚−1h𝑟−1

C. 𝑚𝑜𝑙 𝑙𝑖𝑡−1𝑚𝑖𝑛−1

D. 𝑚𝑜𝑙 𝑐𝑚−3𝑠𝑒𝑐−1

8 / 50

8. Which of the following can be classified as a weak base?

A. None of these

B. Both CH3NH2 and NH2OH

C. CH3NH2

D. NH2OH

9 / 50

9. Does temperature changes affect the equilibrium constant of a reaction?

A. No it does

B. Yes it doesn't

C. Yes it does

D. No it doesn't

10 / 50

10.

A catalyst increases the rate of reaction by providing a different reaction pathway that

A. Lowers only the activation Energy

B. Lowers only the energy of the reactants and products

C. Raises only the energy of the products

D. All of these are affected by the presence of a catalyst

11 / 50

11. The powers to which the concentration of each reactant is raised to give a correct dependence of rate on concentration is termed

A. Equilibrium Law

B. Order of reaction

C. Rate Equation

D. Molecularity of reaction

12 / 50

12. Who is the Dean of Faculty of Science in Fuoye

A. Dr. Lawal

B. Dr. Shakirudeen

C. Dr. Malomo

D. Dr. Okolo

13 / 50

13.

During an electrochemical reaction, electrons move through the external circuit toward the __________ and positive ion in the cell move toward the ____________.

A. Cathode, cathode

B. Anode, anode

C. Anode, cathode

D. Cathode, anode

14 / 50

14. Zinc and carbon rods are used as anode and cathode respectively in a

A. Daniel cell

B. Leclanche cell

C. voltaic cell

D. lead accumulator

15 / 50

15. A reaction in which the same substance on the reactant side is being oxidized and reduced simultaneously is known as

A. Substitution reaction

B. Dispropornation reaction

C. Addition reaction

D. Combustion reaction

16 / 50

16. To balance a redox reaction in basic medium, 𝐻2𝑂 is added to the side with

A. Equivalent number of oxygen atoms

B. More oxygen atoms

C. Lesser number of hydrogen atoms

D. Lesser number of oxygen atoms

17 / 50

17. 1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁷, 4s²
An element with the electronic configuration above is a

A. Metal

B. Group 2 element

C. Transition Element

D. Non metal

18 / 50

18. Elements in a periodic group have similar

A. Chemical properties

B. Physical properties

C. Masses

D. Densities

19 / 50

19. The solution that will conduct the highest amount of electricity is

A. 0.5 mol dm-3 of hydrochloric acid

B. 2.0 mol dm-3 of hydrochloric acid

C. 0.5 mol dm-3 ethanoic acid

D. 2.0 mol dm-3 ethanoic acid

20 / 50

20. How many grams of nickel metal are plated out when a constant current of 15.0A is passed through aqueous NiCl2 for 80.0 minutes

A. 43.8g

B. 14.7g

C. 21.9g

D. 48.4g

21 / 50

21. Substances that dissolve in water to release hydroxonium ion is known as

A. Salt

B. Acid

C. Base

D. Lewis Base

22 / 50

22. Molarity is defined as ______

A. Moles of solvent per liter of solution

B. Moles of solute per litre of solvent

C. Moles solvent per liter of solvent

D. Moles of solute per liter of solution

23 / 50

23. Isotopes have the same number of __________ but different numbers of ___________ in their nuclei

A. Nucleon, neutron

B. Protons, neutrons

C. Protons, electrons

D. Electron, neutron

24 / 50

24.

What is the minimum energy barrier that must be overcome for a chemical reaction to occur

A. Potential Energy

B. Rate limiting energy

C. Net energy

D. Activation Energy

25 / 50

25. The energy of motion is

A. Electrical Energy

B. Reserve energy

C. Dam energy

D. Kinetic Energy

26 / 50

26. Water is best described as

A. Acid

B. Amphoteric

C. Ampiteric

D. Base

27 / 50

27. The number of nucleons in an atom or ion is the same as the

A. Atomic Number

B. None of these

C. Mass Number

D. Charge on the atom or ion

28 / 50

28. A saturated solution is defined as

A. A concentrated solution

B. A solution that is in equilibrium with pure solute

C. A solution that is not in equilibrium with both pure solvent and undissolved solute

D. A solution that is in equilibrium with undisolved solute

29 / 50

29. The unit of rate constant, K, in a first order reaction is

A. 𝑚𝑜𝑙𝑙𝑖𝑡𝑟𝑒−1𝑠𝑒𝑐−1

B. 𝑙𝑖𝑡𝑟𝑒𝑚𝑜𝑙−1𝑠𝑒𝑐−1

C. 𝑠𝑒𝑐−1

D. 𝑠𝑒𝑐𝑙𝑖𝑡𝑟𝑒−1𝑚𝑜𝑙−1

30 / 50

30. Catalyst speeds up the rate of

A. Both forward and reverse reaction

B. Forward Reaction

C. Reverse Reaction

D. All reactions

31 / 50

31. What is the overall reaction order for the reaction that has the rate law: k[H2] [NO] 2

A. First order

B. Third order

C. Zero order

D. Second order

32 / 50

32. How many grams of chromium metal are plated out when a constant current of 8.00A is passed through an aqueous solution containing Cr3+ ions for 40 minutes

A. 10.3g

B. 3.45g

C. 6.15g

D. 31.0g

33 / 50

33. What mass of HNO3(63g/mol) is contained in 300ml of 0.30 M HNO3 solution!

A. 0.3g

B. 6.3g

C. 5.67g

D. 30g

34 / 50

34. What is the electronic configuration of Potassium (K)?

A. 1s2 2s2 2p6 3s2 3p6

B. 1s2 2s2 2p6 3s2

C. 1s2 2s2 2p6 3s2 3p6 4s1

D. 1s2 2s2 2p6

35 / 50

35. The pH of pure water is

A. 7

B. -14

C. -7

D. 14

36 / 50

36. A zeroth order reaction is one whose

A. Rate is dependent on none of the reactants

B. Rate can be found where [A] t =-kt + ln[A] o

C. Rate is independent of reactant concentration

D. Rate is zero

37 / 50

37. The number of molecules/ions of the reactants present in the balanced stoichiometric equation is referred to as:

A. Equilibrium Law

B. Rate Equation

C. Molecularity of reaction

D. Order of reaction

38 / 50

38. The rate of a reaction is directly proportional to the concentration of reactants. This is referred to as

A. Order of a Reaction

B. Overall order of a Reaction

C. Rate of a Reaction

D. Molecularity of a Reaction

39 / 50

39.

An isotope has a half-life of 30 minutes. Given an original sample of 100 g of the isotope, how much will be left after an hour?

A. 25 grams

B. 50 grams

C. 0 grams

D. 100 grams

40 / 50

40. Elements P, Q, R, S have 6, 11, 15, 17 electrons respectively, therefore,

A. Q will form an electrovalent bond with S

B. P will form an electrovalent bond with R

C. Q will form a covalent bond with S

D. R will form an electrovalent bond with S

41 / 50

41. An element that has the valence electronic configuration 3s2 3p3 belongs to which period and group?

A. Period 3 And Group 5A

B. Period 4 and Group 5A

C. Period 3 And Group 3A

D. Period 4 and Group 3A

42 / 50

42. The binding energy is defined as

A. The amount of energy absorbed when protons and neutrons form a nucleus

B. The amount of energy released when electrons are removed from the atom

C. The amount of energy required to break apart a nucleus into individual protons and neutrons

D. The amount of energy absorbed when electrons are added to an ion

43 / 50

43. Ozone is unstable, decomposing to oxygen, as shown in the balanced equation 2O2 ➡ 3O2. In this reaction, how many grams of oxygen can be formed from the decomposition of 96g of ozone?

A. 32g

B. 16g

C. 96g

D. 6g

44 / 50

44. Order of a given reaction can only be determined

A. From the Rate Equation

B. From the Molecuarity of reaction

C. From the chemical reaction

D. Experimentally

45 / 50

45.

Which of the following can be interpreted as a measure of randomness

A. Temperature

B. Entropy

C. Free Energy

D. Enthalpy

46 / 50

46. What is the Mass number of Na?

A. 22

B. 23

C. 11

D. 20

47 / 50

47. What is the pH of a neutral solution at 25 0C?

A. 1

B. 3

C. 7

D. 14

48 / 50

48. The half-life of a first order reaction depends on

A. Initial concentration of the reactants

B. Concentration of the reactant left

C. Concentration of product

D. Rate constant

49 / 50

49. Radiation is detected by its ___________ properties

A. Thermal

B. Ionizing

C. Kinetic

D. Gravitational

50 / 50

50. What is the oxidation number of the chromium atom in K2Cr2O7

A. +3

B. +6

C. +7

D. -2

Your score is

The average score is 28%

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