Home CBT TEST CHM 101 TYPE B CBT PRACTICE TEST

CBT TEST

CHM 101 TYPE B CBT PRACTICE TEST

Phil

March 27, 2023

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
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

Please do well to use our comment box incase there’s a message you want to pass to us

70 – 100 A

60 – 69 B

50 – 59 C

45 – 49 D

40 – 44 E

0 – 39 F

I wish you success

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CHM 101 TYPE B

1 / 40

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

Mg =24.31

N= 14.01

O= 16

A. 0.01889%

B. 1.889%

C. 18.99%

D. 0.1889%

2 / 40

2. 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. Molecularity of reaction

D. Rate Equation

3 / 40

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

A. +3

B. +6

C. -2

D. +7

4 / 40

4. Gamma radiation can be described as

A. High energy electromagnetic radiation

B. positively charged free electron

C. A negatively charged free electron

D. A helium nucleus

5 / 40

5. Water is best described as

A. Ampiteric

B. Amphoteric

C. Base

D. Acid

6 / 40

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

A. Lesser number of oxygen atoms

B. More oxygen atoms

C. Equivalent number of oxygen atoms

D. Lesser number of hydrogen atoms

7 / 40

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

A. Exclusion Principle

B. Le-Chatelier Principle

C. Pauli’s Exclusion Principle

D. Aufbau Principle

8 / 40

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

A. No it doesn't

B. Yes it doesn't

C. Yes it does

D. No it does

9 / 40

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

A. Molecularity of reaction

B. Rate Equation

C. Equilibrium Law

D. Order of reaction

10 / 40

10. Rate of a reaction is measured in

A. 𝑚𝑜𝑙 𝑙𝑖𝑡−1𝑚𝑖𝑛−1

B. 𝑚𝑜𝑙 𝑐𝑚−1h𝑟−1

C. 𝑚𝑜𝑙 𝑐𝑚−3𝑠𝑒𝑐−1

D. 𝑚𝑜𝑙 𝑐𝑚−1𝑠𝑒𝑐−3

11 / 40

11. 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. 6g

C. 96g

D. 16g

12 / 40

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

A. Dalton but not accepted till Mendelev

B. Dalton but not accepted until the work of Einstein

C. Democritus but not widely accepted till modern times

D. Dalton and widely accepted within a few decades

13 / 40

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

A. 30g

B. 5.67g

C. 0.3g

D. 6.3g

14 / 40

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

A. 𝑠𝑒𝑐−1

B. 𝑙𝑖𝑡𝑟𝑒𝑚𝑜𝑙−1𝑠𝑒𝑐

C. 𝑠𝑒𝑐𝑙𝑖𝑡𝑟𝑒−1𝑚𝑜𝑙−1

D. 𝑚𝑜𝑙𝑙𝑖𝑡𝑟𝑒−1𝑠𝑒𝑐−1

15 / 40

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

A. Number of moles

B. Electronic configuration

C. Pressure

D. Temperature

16 / 40

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

A. Rate constant

B. Concentration of the reactant left

C. Concentration of product

D. Initial concentration of the reactions

17 / 40

17. 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. Rate of a Reaction

D. Order of a Reaction

18 / 40

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

A. Order of reaction

B. Rate Equation

C. Molecularity of reaction

D. Equilibrium Law

19 / 40

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

A. increases/lowering

B. decreases/raising

C. decreases/lowering

D. increases/raising

20 / 40

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

A. Dispropornation reaction

B. Substitution reaction

C. Addition reaction

D. Combustion reaction

21 / 40

21. Order of a given reaction can only be determined

A. Experimentally

B. From the Rate Equation

C. From the Molecuarity of reaction

D. From the chemical reaction

22 / 40

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

A. 1

B. 5

C. 4

D. 9

23 / 40

23. A zeroth order reaction is one whose

A. Rate is zero

B. Rate is dependent on none of the reactants

C. Rate is independent of reactant concentration

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

24 / 40

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

A. Fuel Cell

B. Concentration cell

C. Electrolytic Cell

D. Galvanic cell

25 / 40

25. The change in the concentration of reactant or product per unit time is known as

A. Order of a reaction

B. Rate of a reaction

C. Rate Law

D. Molecularity of a reaction

26 / 40

26. 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. Zeroth

C. Fourth

D. First

27 / 40

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

A. 𝑠𝑒𝑐𝑙𝑖𝑡𝑟𝑒−1𝑚𝑜𝑙−1

B. 𝑚𝑜𝑙𝑙𝑖𝑡𝑟𝑒−1𝑠𝑒𝑐−1

C. 𝑠𝑒𝑐−1

D. 𝑙𝑖𝑡𝑟𝑒𝑚𝑜𝑙−1𝑠𝑒𝑐−1

28 / 40

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

A. Base

B. Salt

C. Lewis Base

D. Acid

29 / 40

29. What symbol is used to express the facor,10^-6?

A. µ

B. m

C. M

D. n

30 / 40

30. 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 equilibrium law

D. Overall molecularity of reaction

31 / 40

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

A. Base

B. Acid

C. Lewis Acid

D. Salt

32 / 40

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

A. N

B. Al

C. Mg

D. C

33 / 40

33. 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 3A

D. Period 4 and Group 5A

34 / 40

34. A saturated solution is defined as

A. A concentrated solution

B. A solution that is in equilibrium with undisolved solute

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

D. A solution that is in equilibrium with pure solute

35 / 40

35. The pH of pure water is

A. -7

B. 7

C. -14

D. 14

36 / 40

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

A. 3

B. 1

C. 14

D. 7

37 / 40

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

A. Concentration of the reactant left

B. Rate constant

C. Concentration of product

D. Initial concentration of the reactants

38 / 40

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

A. Net Energy

B. Rate Limiting Energy

C. Activation Energy

D. Potential Energy

39 / 40

39. Catalyst speeds up the rate of

A. All reactions

B. Reverse Reaction

C. Forward Reaction

D. Both forward and reverse reaction

40 / 40

40. Photolytic reactions take place in the presence of

A. Pressure

B. Catalyst

C. Heat

D. Light

Your score is

The average score is 46%

CHM 101 TYPE B CBT PRACTICE TEST

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