CHM 101 TYPE B CBT PRACTICE TEST : Undergragra

Warning: Undefined array key "HTTP_SEC_FETCH_SITE" in /home/undergra/public_html/wp-content/plugins/quiz-maker/includes/class-quiz-maker-iframe.php on line 71

Warning: Undefined array key "HTTP_SEC_FETCH_SITE" in /home/undergra/public_html/wp-content/plugins/quiz-maker/includes/class-quiz-maker-iframe.php on line 71

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

Join The General Freshers Group

https://chat.whatsapp.com/LIwcrkishgH6BsELwcW5w2

Join Undergragra Campus Update Channel

Whatsapp: https://whatsapp.com/channel/0029VakX28dFi8xdORrhjI34

Telegram: https://t.me/ugchannel

I remain your favoVrite education blogger

❤️ Undergragra

0 votes, 0 avg

2747

Created on March 27, 2023 By

Aruwaji Philip

CHM 101 TYPE B

1 / 40

1. Photolytic reactions take place in the presence of

A. Pressure

B. Heat

C. Light

D. Catalyst

2 / 40

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

A. Order of reaction

B. Molecularity of reaction

C. Rate Equation

D. Equilibrium Law

3 / 40

3. 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. 96g

B. 6g

C. 16g

D. 32g

4 / 40

4. A saturated solution is defined as

A. A solution that is in equilibrium with pure solute

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 concentrated solution

5 / 40

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

A. Temperature

B. Electronic configuration

C. Number of moles

D. Pressure

6 / 40

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

A. +6

B. +3

C. +7

D. -2

7 / 40

7. 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. Fourth

B. Second

C. First

D. Zeroth

8 / 40

8. Gamma radiation can be described as

A. A negatively charged free electron

B. positively charged free electron

C. A helium nucleus

D. High energy electromagnetic radiation

9 / 40

9. Water is best described as

A. Acid

B. Ampiteric

C. Amphoteric

D. Base

10 / 40

10. A zeroth order reaction is one whose

A. Rate is independent of reactant concentration

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

C. Rate is zero

D. Rate is dependent on none of the reactants

11 / 40

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

A. 5.67g

B. 30g

C. 6.3g

D. 0.3g

12 / 40

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

A. Activation Energy

B. Potential Energy

C. Net Energy

D. Rate Limiting Energy

13 / 40

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

A. Concentration cell

B. Fuel Cell

C. Galvanic cell

D. Electrolytic Cell

14 / 40

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

A. increases/lowering

B. increases/raising

C. decreases/lowering

D. decreases/raising

15 / 40

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

A. Concentration of the reactant left

B. Concentration of product

C. Initial concentration of the reactants

D. Rate constant

16 / 40

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

A. Acid

B. Lewis Acid

C. Base

D. Salt

17 / 40

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

A. C

B. Mg

C. Al

D. N

18 / 40

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

A. Salt

B. Lewis Base

C. Acid

D. Base

19 / 40

19. 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

20 / 40

20. The pH of pure water is

A. -14

B. -7

C. 14

D. 7

21 / 40

21. 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. Democritus but not widely accepted till modern times

C. Dalton but not accepted till Mendelev

D. Dalton and widely accepted within a few decades

22 / 40

22. Catalyst speeds up the rate of

A. Forward Reaction

B. All reactions

C. Both forward and reverse reaction

D. Reverse Reaction

23 / 40

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

A. Exclusion Principle

B. Pauli’s Exclusion Principle

C. Le-Chatelier Principle

D. Aufbau Principle

24 / 40

24. 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

25 / 40

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

A. n

B. M

C. µ

D. m

26 / 40

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

A. 𝑠𝑒𝑐𝑙𝑖𝑡𝑟𝑒−1𝑚𝑜𝑙−1

B. 𝑠𝑒𝑐−1

C. 𝑚𝑜𝑙𝑙𝑖𝑡𝑟𝑒−1𝑠𝑒𝑐−1

D. 𝑙𝑖𝑡𝑟𝑒𝑚𝑜𝑙−1𝑠𝑒𝑐−1

27 / 40

27. 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. Rate Equation

C. Molecularity of reaction

D. Order of reaction

28 / 40

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

A. Concentration of the reactant left

B. Concentration of product

C. Initial concentration of the reactions

D. Rate constant

29 / 40

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

A. Order of a Reaction

B. Rate of a Reaction

C. Molecularity of a Reaction

D. Overall order of a Reaction

30 / 40

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

A. Rate of a reaction

B. Molecularity of a reaction

C. Rate Law

D. Order of a reaction

31 / 40

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

A. 7

B. 1

C. 3

D. 14

32 / 40

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

A. Substitution reaction

B. Addition reaction

C. Dispropornation reaction

D. Combustion reaction

33 / 40

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

A. 9

B. 1

C. 4

D. 5

34 / 40

34. 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 4 and Group 3A

D. Period 3 And Group 3A

35 / 40

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

A. Yes it does

B. Yes it doesn't

C. No it doesn't

D. No it does

36 / 40

36. 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. 0.1889%

D. 18.99%

37 / 40

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

A. Lesser number of hydrogen atoms

B. Equivalent number of oxygen atoms

C. More oxygen atoms

D. Lesser number of oxygen atoms

38 / 40

38. Order of a given reaction can only be determined

A. From the Molecuarity of reaction

B. Experimentally

C. From the Rate Equation

D. From the chemical reaction

39 / 40

39. 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

40 / 40

40. Rate of a reaction is measured in

A. 𝑚𝑜𝑙 𝑙𝑖𝑡−1𝑚𝑖𝑛−1

B. 𝑚𝑜𝑙 𝑐𝑚−1h𝑟−1

C. 𝑚𝑜𝑙 𝑐𝑚−1𝑠𝑒𝑐−3

D. 𝑚𝑜𝑙 𝑐𝑚−3𝑠𝑒𝑐−1

Your score is

The average score is 46%

Related posts:

Office Hours

Stay In Touch