FUOYE CHM 101 CBT PRACTICE TEST EXAM MODE

Ace/Undergragra March 6, 2023

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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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Created on January 07, 2023 By

Ace/Undergragra

CHM 101

1 / 50

The effect of ionizing radiation depend on

A. All of the above

B. Type and energy of radiation

C. Location of source (internal or external)

D. Length of exposure to radiation

2 / 50

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

A. Lowers only the energy of the reactants and products

B. Lowers only the activation Energy

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

D. Raises only the energy of the products

3 / 50

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

A. 0.341g

B. 6.82g

C. 1.71g

D. 3.41g

4 / 50

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

A. NH2OH

B. CH3NH2

C. Both CH3NH2 and NH2OH

D. None of these

5 / 50

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

A. Moderate to heavy

B. Very low

C. Very heavy

D. Moderate

6 / 50

6. Molarity is defined as ______

A. Moles solvent per liter of solvent

B. Moles of solute per litre of solvent

C. Moles of solvent per liter of solution

D. Moles of solute per liter of solution

7 / 50

7. 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. 3.45g

B. 10.3g

C. 6.15g

D. 31.0g

8 / 50

8. Which group reacts violently with water?

A. Alkali metals

B. Halogens

C. Alkaline earth metal

D. Noble gases

9 / 50

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

A. Electron, neutron

B. Protons, neutrons

C. Protons, electrons

D. Nucleon, neutron

10 / 50

10. 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 until the work of Einstein

C. Dalton but not accepted till Mendelev

D. Dalton and widely accepted within a few decades

11 / 50

11. Water is an example of

A. A mixture

B. Compound

C. An element

D. An ion

12 / 50

12. What is the Mass number of Na?

A. 22

B. 11

C. 20

D. 23

13 / 50

13. 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

14 / 50

14. The Element that best describes Alpha decay is?

A. Calcium

B. Helium

C. Methane

D. Sodium

15 / 50

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

A. M

B. m

C. n

D. µ

16 / 50

16. 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

17 / 50

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

A. Electrolytic Cell

B. Concentration cell

C. Fuel Cell

D. Galvanic cell

18 / 50

18.

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, cathode

C. Cathode, anode

D. Anode, anode

19 / 50

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

A. First order

B. Zero order

C. Third order

D. Second order

20 / 50

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

Mg =24.31

N= 14.01

O= 16

A. 18.99%

B. 1.889%

C. 0.1889%

D. 0.01889%

21 / 50

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

A. -2

B. +7

C. +3

D. +6

22 / 50

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

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

B. 1s2 2s2 2p6

C. 1s2 2s2 2p6 3s2

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

23 / 50

23. Gamma radiation can be described as

A. A negatively charged free electron

B. positively charged free electron

C. High energy electromagnetic radiation

D. A helium nucleus

24 / 50

24. A saturated solution is defined as

A. A solution that is in equilibrium with undisolved solute

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

C. A concentrated solution

D. A solution that is in equilibrium with pure solute

25 / 50

25. Radiation is detected by its ___________ properties

A. Kinetic

B. Thermal

C. Gravitational

D. Ionizing

26 / 50

26. Elements in a periodic group have similar

A. Chemical properties

B. Physical properties

C. Masses

D. Densities

27 / 50

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

A. Fluorine

B. Chlorine

C. Bromine

D. Iodine

28 / 50

28.

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. 0 grams

C. 50 grams

D. 100 grams

29 / 50

29. The factor 0.001 corresponds to which prefix

A. Milli

B. Deci

C. deka

D. Centi

30 / 50

30.

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

A. Potential Energy

B. Activation Energy

C. Rate limiting energy

D. Net energy

31 / 50

31. Which of the following supports Boyles law

A. T = KV

B. K=PV

C. NRT=KV

D. PV/R

32 / 50

32.

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

A. Free Energy

B. Temperature

C. Entropy

D. Enthalpy

33 / 50

33. Chlorine belongs to the ____________ group on the periodic table

A. Halogen

B. Alkaline earth metal

C. Noble

D. Alkali metal

34 / 50

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

A. Dr. Lawal

B. Dr. Okolo

C. Dr. Shakirudeen

D. Dr. Malomo

35 / 50

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

A. N

B. Al

C. C

D. Mg

36 / 50

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

A. Galvanic cell

B. Concentration cell

C. Fuel Cell

D. Electrolytic Cell

37 / 50

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

A. Number of moles

B. Pressure

C. Temperature

D. Electronic configuration

38 / 50

38. The binding energy is defined as

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

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 released when electrons are removed from the atom

39 / 50

39. 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. 14.7g

B. 43.8g

C. 21.9g

D. 48.4g

40 / 50

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

A. Period 4 and Group 3A

B. Period 4 and Group 5A

C. Period 3 And Group 5A

D. Period 3 And Group 3A

41 / 50

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

A. Atomic Number

B. Charge on the atom or ion

C. Mass Number

D. None of these

42 / 50

42. The energy of motion is

A. Reserve energy

B. Dam energy

C. Electrical Energy

D. Kinetic Energy

43 / 50

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

A. +3

B. -2

C. +6

D. +7

44 / 50

44. A zeroth order reaction is one whose

A. Rate is dependent on none of the reactants

B. Rate is zero

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

D. Rate is independent of reactant concentration

45 / 50

45. What is the mole fraction of ethanol in a solution made by dissolving 25g of ethanol, C2H5OH, in 53.6g of Water

A. 0.154

B. 0.214

C. 0.846

D. 0.272

46 / 50

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

A. Activation Energy

B. Rate Limiting Energy

C. Net Energy

D. Potential Energy

47 / 50

47.

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

A. -0.93°C

B. -2.8°C

C. -6.5°C

D. -1.9°C

48 / 50

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

A. Pb(OH)2

B. AgBr

C. Na2SO4

D. PbCrO4

49 / 50

49. Which of the following is not an Arrhenius acid?

A. KOH

B. HF

C. H2SO3

D. HCLO

50 / 50

50. 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

Your score is

The average score is 48%