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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.

Take your time to read instructions before taking this test.

There are 50 questions which you are to answer in 20 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

Note

Do not be in a hurry to answer the questions

Do not waste time on a question you don’t know

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

Always crosscheck

Don’t be in a hurry to submit, you are not in a competition

Don’t be scared. Getting an A is easy

Don’t be over confident, you can end up a D, E or F. Calm your blood, no be only you sabi book

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/50

Created on April 13, 2025 By

Phil

EKSU CHM 101

1 / 50

1. The pH of pure water is

A. 14

B. -7

C. -14

D. 7

2 / 50

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

A. Non metal

B. Transition Element

C. Group 2 element

D. Metal

3 / 50

3. The binding energy is defined as

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

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

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

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

4 / 50

4. The Element that best describes Alpha decay is?

A. Calcium

B. Sodium

C. Helium

D. Methane

5 / 50

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

A. +6

B. +7

C. -2

D. +3

6 / 50

6. Water is best described as

A. Acid

B. Amphoteric

C. Ampiteric

D. Base

7 / 50

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

A. Dr. Lawal

B. Dr. Malomo

C. Dr. Shakirudeen

D. Dr. Okolo

8 / 50

8. 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 order of reaction

C. Overall molecularity of reaction

D. Overall equilibrium law

9 / 50

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

A. Q will form a covalent bond with S

B. R will form an electrovalent bond with S

C. Q will form an electrovalent bond with S

D. P will form an electrovalent bond with R

10 / 50

10. The ion that can be used as an oxidizing agent is

A. Fe3+

B. Ca2+

C. Au3+

D. F-

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. Order of reaction

B. Equilibrium Law

C. Rate Equation

D. Molecularity of reaction

12 / 50

12. Catalyst ................... the rate of reaction by ................... the activation energy

A. decreases/lowering

B. increases/raising

C. increases/lowering

D. decreases/raising

13 / 50

13.

What is the expected freezing point of a 0.50m solution of Na2CO3 in water? Kf for water is 1.86°C/m

A. -1.9°C

B. -6.5°C

C. -0.93°C

D. -2.8°C

14 / 50

14. 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. 48.4g

B. 21.9g

C. 43.8g

D. 14.7g

15 / 50

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

A. Molecularity of a Reaction

B. Overall order of a Reaction

C. Order of a Reaction

D. Rate of a Reaction

16 / 50

16. Molarity is defined as ______

A. Moles of solute per litre of solvent

B. Moles of solvent per liter of solution

C. Moles solvent per liter of solvent

D. Moles of solute per liter of solution

17 / 50

17. Radiation is detected by its ___________ properties

A. Thermal

B. Ionizing

C. Kinetic

D. Gravitational

18 / 50

18. According to history, the concept that all matter is composed of atom was first proposed by

A. Democritus but not widely accepted till modern times

B. Dalton but not accepted till Mendelev

C. Dalton and widely accepted within a few decades

D. Dalton but not accepted until the work of Einstein

19 / 50

19.

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

A. Net energy

B. Rate limiting energy

C. Activation Energy

D. Potential Energy

20 / 50

20.

The effect of ionizing radiation depend on

A. Location of source (internal or external)

B. Type and energy of radiation

C. All of the above

D. Length of exposure to radiation

21 / 50

21. What is the identity of the element with 6 protons, 7 Neutrons and 6 electrons

A. N

B. Al

C. Mg

D. C

22 / 50

22. The factor 0.001 corresponds to which prefix

A. Milli

B. Deci

C. Centi

D. deka

23 / 50

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

A. 6.3g

B. 30g

C. 0.3g

D. 5.67g

24 / 50

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

A. 2.0 mol dm-3 ethanoic acid

B. 0.5 mol dm-3 ethanoic acid

C. 2.0 mol dm-3 of hydrochloric acid

D. 0.5 mol dm-3 of hydrochloric acid

25 / 50

25. What is the oxidation number of the chromium atom in K2Cr2O4?

A. +3

B. +7

C. +6

D. -2

26 / 50

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

A. Period 3 And Group 5A

B. Period 3 And Group 3A

C. Period 4 and Group 5A

D. Period 4 and Group 3A

27 / 50

27. Rate of a reaction is measured in

A. 𝑚𝑜𝑙 𝑐𝑚−3𝑠𝑒𝑐−1

B. 𝑚𝑜𝑙 𝑐𝑚−1𝑠𝑒𝑐−3

C. 𝑚𝑜𝑙 𝑐𝑚−1h𝑟−1

D. 𝑚𝑜𝑙 𝑙𝑖𝑡−1𝑚𝑖𝑛−1

28 / 50

28.

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

A. Entropy

B. Temperature

C. Enthalpy

D. Free Energy

29 / 50

29. What is the minimum energy barrier that must be overcomed for a chemical reaction to occur

A. Activation Energy

B. Rate Limiting Energy

C. Potential Energy

D. Net Energy

30 / 50

30. Elements with ___________ atomic mass are best possible candidates for a fusion reaction

A. Very low

B. Moderate

C. Moderate to heavy

D. Very heavy

31 / 50

31. The shifting of the equilibrium position to annul the effect of changes to re-establish equilibrium is termed

A. Exclusion Principle

B. Aufbau Principle

C. Le-Chatelier Principle

D. Pauli’s Exclusion Principle

32 / 50

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

A. Rate constant

B. Concentration of product

C. Concentration of the reactant left

D. Initial concentration of the reactants

33 / 50

33.

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

A. Cathode, anode

B. Anode, cathode

C. Anode, anode

D. Cathode, cathode

34 / 50

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

A. 1s2 2s2 2p6 3s2

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

C. 1s2 2s2 2p6

D. 1s2 2s2 2p6 3s2 3p6

35 / 50

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

A. 𝑙𝑖𝑡𝑟𝑒𝑚𝑜𝑙−1𝑠𝑒𝑐−1

B. 𝑚𝑜𝑙𝑙𝑖𝑡𝑟𝑒−1𝑠𝑒𝑐−1

C. 𝑠𝑒𝑐−1

D. 𝑠𝑒𝑐𝑙𝑖𝑡𝑟𝑒−1𝑚𝑜𝑙−1

36 / 50

36. Catalyst speeds up the rate of

A. All reactions

B. Reverse Reaction

C. Both forward and reverse reaction

D. Forward Reaction

37 / 50

37. A saturated solution is defined as

A. A concentrated solution

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

C. A solution that is in equilibrium with undisolved solute

D. A solution that is in equilibrium with pure solute

38 / 50

38. Which of the following compounds would be soluble in water?

A. Pb(OH)2

B. PbCrO4

C. Na2SO4

D. AgBr

39 / 50

39. 2C₂H_2(g) + 5O_2(g) → 4CO_2(g) + 2H₂O_(g)
In the reaction above, the mass of carbon(IV)oxide produced on burning 78 g of ethyne is
[C =12, O = 16, H = 1]

A. 264g

B. 156g

C. 352g

D. 39g

40 / 50

40. Which cell involves a non-spontaneous redox reaction?

A. Fuel Cell

B. Electrolytic Cell

C. Concentration cell

D. Galvanic cell

41 / 50

41. Of the following, which element has the highest first ionization energy

A. Iodine

B. Bromine

C. Fluorine

D. Chlorine

42 / 50

42. Which of the following supports Boyles law

A. K=PV

B. PV/R

C. T = KV

D. NRT=KV

43 / 50

43. A substance that ionizes in solution to produce hydroxyl ion is

A. Base

B. Lewis Acid

C. Salt

D. Acid

44 / 50

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

A. Protons, neutrons

B. Nucleon, neutron

C. Electron, neutron

D. Protons, electrons

45 / 50

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

A. 14

B. 3

C. 7

D. 1

46 / 50

46. Water is an example of

A. An element

B. Compound

C. An ion

D. A mixture

47 / 50

47. An element with atomic number twelve is likely to be

A. covalent with a valency of 2

B. electrovalent with a velocity of 1

C. electrovalent with a valency of 2

D. covalent with a valency of 4

48 / 50

48. Elements in a periodic group have similar

A. Densities

B. Physical properties

C. Chemical properties

D. Masses

49 / 50

49. Gamma radiation can be described as

A. positively charged free electron

B. A helium nucleus

C. A negatively charged free electron

D. High energy electromagnetic radiation

50 / 50

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

A. Lesser number of hydrogen atoms

B. Lesser number of oxygen atoms

C. More oxygen atoms

D. Equivalent number of oxygen atoms

Your score is

The average score is 7%

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EKSU CHM 101 CBT PRACTICE

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