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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 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

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

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Created on April 24, 2025 By

Phil

EBSU CHM 101

1 / 50

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

A. PbCrO4

B. Na2SO4

C. AgBr

D. Pb(OH)2

2 / 50

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

A. 5.67g

B. 30g

C. 0.3g

D. 6.3g

3 / 50

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

A. Dr. Shakirudeen

B. Dr. Lawal

C. Dr. Okolo

D. Dr. Malomo

4 / 50

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

A. None of these

B. Mass Number

C. Atomic Number

D. Charge on the atom or ion

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

A. decreases/lowering

B. decreases/raising

C. increases/raising

D. increases/lowering

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6. 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

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

A. Electrolytic Cell

B. Fuel Cell

C. Concentration cell

D. Galvanic cell

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

A. Aufbau Principle

B. Exclusion Principle

C. Pauli’s Exclusion Principle

D. Le-Chatelier Principle

9 / 50

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

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10. 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. 352g

B. 156g

C. 39g

D. 264g

11 / 50

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

A. 14

B. 7

C. 3

D. 1

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

A. Dalton but not accepted until the work of Einstein

B. Dalton and widely accepted within a few decades

C. Dalton but not accepted till Mendelev

D. Democritus but not widely accepted till modern times

13 / 50

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

A. Concentration of the reactant left

B. Initial concentration of the reactants

C. Rate constant

D. Concentration of product

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14. If 30cm³ of gas at 50^oC is warmed to 80^o at a fixed pressure, the fractional increase in volume is

A. 0.910

B. 0.093

C. 1.090

D. 0.009

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

A. Both CH3NH2 and NH2OH

B. NH2OH

C. CH3NH2

D. None of these

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

A. Molecularity of reaction

B. Equilibrium Law

C. Order of reaction

D. Rate Equation

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17.

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

A. Free Energy

B. Enthalpy

C. Temperature

D. Entropy

18 / 50

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

A. Initial concentration of the reactions

B. Concentration of product

C. Concentration of the reactant left

D. Rate constant

19 / 50

19. Which group reacts violently with water?

A. Noble gases

B. Halogens

C. Alkali metals

D. Alkaline earth metal

20 / 50

20. Which of the following is not used to describe the condition of a gas?

A. Pressure

B. Electronic configuration

C. Temperature

D. Number of moles

21 / 50

21.

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

A. -2.8°C

B. -1.9°C

C. -0.93°C

D. -6.5°C

22 / 50

22. Radiation is detected by its ___________ properties

A. Kinetic

B. Ionizing

C. Gravitational

D. Thermal

23 / 50

23. Water is an example of

A. An element

B. A mixture

C. An ion

D. Compound

24 / 50

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

A. Al

B. Mg

C. N

D. C

25 / 50

25. Using the method of initial rates for the reaction A➡B, if the initial concentration of A is doubled and the rate of reaction quadruples, what is the order of reaction with respect to A?

A. Second

B. Fourth

C. Zeroth

D. First

26 / 50

26. A saturated solution is defined as

A. A solution that is in equilibrium with undisolved solute

B. A concentrated solution

C. A solution that is in equilibrium with pure solute

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

27 / 50

27. 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

28 / 50

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

A. Fe3+

B. Au3+

C. Ca2+

D. F-

29 / 50

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

A. Protons, electrons

B. Protons, neutrons

C. Electron, neutron

D. Nucleon, neutron

30 / 50

30. 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. 6g

B. 16g

C. 96g

D. 32g

31 / 50

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

A. -2

B. +6

C. +3

D. +7

32 / 50

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

A. Very low

B. Very heavy

C. Moderate to heavy

D. Moderate

33 / 50

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

Mg =24.31

N= 14.01

O= 16

A. 0.1889%

B. 0.01889%

C. 18.99%

D. 1.889%

34 / 50

34. Which of the following supports Boyles law

A. PV/R

B. NRT=KV

C. K=PV

D. T = KV

35 / 50

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

A. covalent with a valency of 4

B. electrovalent with a valency of 2

C. covalent with a valency of 2

D. electrovalent with a velocity of 1

36 / 50

36.

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

37 / 50

37. 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. Rate Equation

C. Molecularity of reaction

D. Equilibrium Law

38 / 50

38. How many grams of KNO3 are needed to make 250ML of a solution that is 0.135M

A. 0.341g

B. 6.82g

C. 3.41g

D. 1.71g

39 / 50

39. What is the pH of a basic solution whose hydroxyl ion concentration is 0.00001M?

A. 1

B. 5

C. 9

D. 4

40 / 50

40. 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

41 / 50

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

A. voltaic cell

B. Daniel cell

C. lead accumulator

D. Leclanche cell

42 / 50

42. Rate of a reaction is measured in

A. 𝑚𝑜𝑙 𝑐𝑚−1𝑠𝑒𝑐−3

B. 𝑚𝑜𝑙 𝑐𝑚−3𝑠𝑒𝑐−1

C. 𝑚𝑜𝑙 𝑙𝑖𝑡−1𝑚𝑖𝑛−1

D. 𝑚𝑜𝑙 𝑐𝑚−1h𝑟−1

43 / 50

43. The binding energy is defined as

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

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

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

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

44 / 50

44. Order of a given reaction can only be determined

A. From the Rate Equation

B. Experimentally

C. From the Molecuarity of reaction

D. From the chemical reaction

45 / 50

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

A. Acid

B. Base

C. Salt

D. Lewis Base

46 / 50

46. Elements in a periodic group have similar

A. Physical properties

B. Chemical properties

C. Masses

D. Densities

47 / 50

47. Gamma radiation can be described as

A. High energy electromagnetic radiation

B. A negatively charged free electron

C. positively charged free electron

D. A helium nucleus

48 / 50

48. The Element that best describes Alpha decay is?

A. Helium

B. Calcium

C. Methane

D. Sodium

49 / 50

49.

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

A. Net energy

B. Potential Energy

C. Activation Energy

D. Rate limiting energy

50 / 50

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

A. Overall equilibrium law

B. Overall rate law

C. Overall order of reaction

D. Overall molecularity of reaction

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The average score is 28%

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