Fundamentals Chapter.1 Verified Test Bank

Chapter 1: Fundamentals

Test Bank

Type: fill-in-blank

Title: Chapter 01 Question 01

1) Systeme International d’Unites is the internationally recognised system of metric units. The system has _____ base units from which all other SI units can be derived.

Section reference: 1.2

a. seven

Type: multiple response question

Title: Chapter 01 Question 02

2) The H-Cl bond length is 127.5 pm. Which of the following lengths is equivalent? Please select all that apply.

Section reference: 1.2

a. 1.275 × 10^-12 m.

b. 1.275 Å.

c. 0.1275 nm.

d. 1.275 × 10^-10 mm.

Type: matching question

Title: Chapter 01 Question 03

3) Chemists commonly use the Kelvin (T / K) and Celsius (θ / °C) temperature scales. Match the values in Celsius to the equivalent value on the kelvin temperature scale.

Section reference: 1.2

a. 100 °C = 373.15 K

b. 0 °C = 273.15 K

c. -273.15 °C = 0 K

d. 25 °C = 298 K

Type: multiple choice question

Title: Chapter 01 Question 04

4) The derived SI unit for pressure is Pa (pascals). What is this in base SI units given that pressure = force/area?

a. atm.

Section reference: 1.2

b. Kg m^-1 s^-2.

Section reference: 1.2

c. bar.

Section reference: 1.2

d. g mm^-1 s^-2.

Section reference: 1.2

Type: multiple response question

Title: Chapter 01 Question 05

5) Which of the following will the isotopes of an element have in common? Please select all that apply.

Section reference: 1.3

a. The same number of protons.

b. The same number of neutrons.

c. A different number of electrons.

d. A different number of neutrons.

Type: multiple choice question

Title: Chapter 01 Question 06

6) Element X has the atomic symbol. How many neutrons are there in the nucleus?

a. 18.

Section reference: 1.3

b. 36.

Section reference: 1.3

c. 22.

Section reference: 1.3

d. 40.

Section reference: 1.3

Type: true-false

Title: Chapter 01 Question 07

7) Isotopes of an element chemically react in the same manner but differ in their physical properties.

a. True

Section reference: 1.3

b. False

Section reference: 1.3

Type: fill-in-blank

Title: Chapter 01 Question 08

8) The number of atoms of xenon in 1 mole is equal to _________ constant.

Section reference: 1.3

a. Avogadro’s

Type: multiple choice question

Title: Chapter 01 Question 09

9) What mass (in g) of gold contains 8.9 mol of Au?

a. 12 g.

Section reference: 1.3

b. 0.045 g.

Section reference: 1.3

c. 1753.033 g.

Section reference: 1.3

d. 6.022 × 10²³ g.

Section reference: 1.3

Type: multiple choice question

Title: Chapter 01 Question 10

10) How many moles of molecules are contained in 232 g of SiO₂?

a. 0.26 mol.

Section reference: 1.3

b. 3.86 mol.

Section reference: 1.3

c. 13939.49 mol.

Section reference: 1.3

d. 5.26 mol.

Section reference: 1.3

Type: fill-in-blank

Title: Chapter 01 Question 11

11) An organic compound is found to contain by mass, 76.57% carbon, 6.43% hydrogen and 17% oxygen and a relative molecular mass (M_r) of 94.12 g mol^-1. The molecular formula of the compound is ______.

Section reference: 1.3

a. C₆H₆O₁.

Type: true-false

Title: Chapter 01 Question 12

12) The empirical formula of a substance tells you the actual number of different elements in a molecule.

a. True

Section reference: 1.3

b. False

Section reference: 1.3

Type: multiple response question

Title: Chapter 01 Question 13

13) The combustion of glucose in a plentiful of supply of air is given by the following equation: W C₆H₁₂O₆ (s) + X O₂(g) → Y CO₂ (g) + Z H₂O (l). What are the values of the stoichiometric coefficients W, X, Y, and Z?

Please select all that apply.

Section reference: 1.4

a. W = 2.

b. X = 6.

c. Y = 6.

d. Z = 6.

Type: multiple choice question

Title: Chapter 01 Question 14

14) The balanced equation for the combustion of sucrose in a plentiful supply of air is: C₁₂H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l). What mass of oxygen is needed to react exactly with 500 g of sucrose?

a. 6000 g.

332.22 g 383.98 g

1 g g

500 g = 577.90 g = 578 g.

Section reference: 1.4

b. 578 g.

332.22 g 383.98 g

1 g g

500 g = 577.90 g = 578 g.

Section reference: 1.4

c. 384 g.

332.22 g 383.98 g

1 g g

500 g = 577.90 g = 578 g.

Section reference: 1.4

d. 500 g.

332.22 g 383.98 g

1 g g

500 g = 577.90 g = 578 g.

Section reference: 1.4

Type: multiple choice question

Title: Chapter 01 Question 15

15) What is the oxidation state of C in Li₂CO₃?

a. +1.

Section reference: 1.4

b. +2.

Section reference: 1.4

c. +3.

Section reference: 1.4

d. +4.

Section reference: 1.4

Type: multiple choice question

Title: Chapter 01 Question 16

16) What is the oxidation state of N in KNO₂?

a. +1.

Section reference: 1.4

b. +2.

Section reference: 1.4

c. +3.

Section reference: 1.4

d. +4.

Section reference: 1.4

Type: fill-in-blank

Title: Chapter 01 Question 17

17) In the reaction of lithium with water lithium has been ________.

2 Li(s) + 2 H₂O(l) → 2 LiOH(aq) + H₂(g)

Section reference: 1.4

a. oxidised

Type: fill-in-blank

Title: Chapter 01 Question 18

18) The systematic name for SF₆ is sulphur ____fluoride

Section reference: 1.4

a. hexa

Type: matching question

Title: Chapter 01 Question 19

19) Match the following brief description with the correct term:

Section reference: 1.4

a. involves the transfer of a proton = Acid-base reaction

b. involves the formation of a solid product when two solutions are mixed = Precipitation reaction

c. involves the transfer of electrons = Redox reaction

d. involves the formation of a complex = Complexation reaction

Type: fill-in-blank

Title: Chapter 01 Question 20

20) The systematic name for XeF₄ is xenon _____fluoride

a. tetra

Type: fill-in-blank

Title: Chapter 01 Question 21

21) The systematic name for SiO₂ is silicon __oxide

Section reference: 1.4

a. di

Type: multiple choice question

Title: Chapter 01 Question 22

22) In the reaction between zinc and hydrogen chloride, what is the oxidation state change of zinc?

Zn (s) + HCl (l) → ZnCl₂ (s) + H₂ (g)

a. +2.

Section reference: 1.4

b. -2.

Section reference: 1.4

c. 0.

Section reference: 1.4

d. +1.

Section reference: 1.4

Type: multiple choice question

Title: Chapter 01 Question 23

23) 23.75 g of potassium iodide was dissolved in water and the solution made up to 250 cm³. What is the concentration of the solution in mol dm^-3?

a. 0.38

Section reference: 1.5

b. 0.57

Section reference: 1.5

c. 95

Section reference: 1.5

d. 0.095

Section reference: 1.5

Type: multiple choice question

Title: Chapter 01 Question 24

24) In order to make a 500 cm³ solution of potassium chloride, concentration 2 mol dm^-3, what mass (in g) of potassium chloride must be dissolved in water?

a. 1 g.

Section reference: 1.3, 1.5

b. 74550 g.

Section reference: 1.3, 1.5

c. 149.10 g.

Section reference: 1.3, 1.5

d. 74.55 g.

Section reference: 1.3, 1.5

Type: multiple response question

Title: Chapter 01 Question 25

25) When the equivalence point of a titration has been reached, the following statements apply. Please select all that apply.

Section reference: 1.5

a. There are equal volumes of reagents.

b. The amount of reagent added from the burette has reacted exactly with the solution in the conical flask.

c. There are equal amounts (mass) of reagents.

d. An indicator added would change colour at this point.

Type: multiple choice question

Title: Chapter 01 Question 26

26) In order to make a 750 cm³ solution of potassium iodate (KIO₃), with concentration 2.5 mol dm^-3, what mass (in g) of potassium iodate must be dissolved?

a. 401 g.

Section reference: 1.3, 1.5

b. 401241 g.

Section reference: 1.3, 1.5

c. 1.875 g.

Section reference: 1.3, 1.5

d. 535 g.

Section reference: 1.3, 1.5

Type: multiple choice question

Title: Chapter 01 Question 27

27) A solution of potassium iodate (KIO₃) has a concentration of 1.75 mol dm^-3. What volume (in dm³) of solution contains exactly 50 g?

a. 1.335 × 10^-4 .

Section reference: 1.3, 1.5

b. 0.134

Section reference: 1.3, 1.5

c. 0.0875

Section reference: 1.3, 1.5

d. 2.45

Section reference: 1.3, 1.5

Type: multiple choice question

Title: Chapter 01 Question 28

28) In a titration, a standard solution of hydrochloric acid (concentration 0.2 mol dm^-3) was added to 25 cm³ of a sodium hydroxide solution, concentration unknown. On addition of 18.5 cm³ HCl, the equivalence point was reached. What is the concentration of the sodium hydroxide solution?

a. 0.2

Section reference: 1.5

b. 3.7 × 10^-3.

Section reference: 1.5

c. 0.296

Section reference: 1.5

d. 0.148

Section reference: 1.5

Type: multiple choice question

Title: Chapter 01 Question 29

29) A 150 cm³ solution containing Br^- was treated with excess AgNO₃ in order to find the Br^- concentration in the solution. 0.873 g of AgBr was precipitated out. What was the concentration (in mol dm^-3) of Br^- in the unknown solution?

a. 4.65 × 10^-3.

Section reference: 1.5

b. 0.031

Section reference: 1.5

c. 3.10 × 10^-5.

Section reference: 1.5

d. 0.073

Section reference: 1.5

Type: multiple choice question

Title: Chapter 01 Question 30

30) A standard solution of Ba(OH)₂ (concentration 0.25 mol dm^-3) was added to 50 cm³ of a HNO₃ solution, concentration unknown. On addition of 28.35 cm³ Ba(OH)₂, the equivalence point was reached. What is the concentration (in mol dm^-3) of the sodium hydroxide solution?

Ba(OH)₂ (aq) + 2 HNO₃ (aq) → Ba(NO₃)₂ (aq) + 2 H₂O (l) a. 0.014

Section reference: 1.5

b. 0.28

Section reference: 1.5

c. 0.25

Section reference: 1.5

d. 7.0875 × 10^-3

Section reference: 1.5

Type: true-false

Title: Chapter 01 Question 31

31) An endothermic reaction is one in which the system releases energy and warms the surroundings.

a. True

Section reference: 1.6

b. False

Section reference: 1.6

Type: fill-in-blank

Title: Chapter 01 Question 32

32) An exothermic reaction has a ________ enthalpy change.

Section reference: 1.6

a. negative

Type: fill-in-blank

Title: Chapter 01 Question 33

33) The enthalpy change of a reaction is the heat transferred between the reaction and its surroundings at constant ________.

Section reference: 1.6

a. pressure

Type: multiple response question

Title: Chapter 01 Question 34

34) What information does this symbol convey about an enthalpy change? Please select all that apply.

Section reference: 1.6

a. is measured at a pressure of 1 atm.

b. is measured at a temperature of 298 K.

c. is measured under standard conditions.

d. is the standard enthalpy change of formation.

Type: multiple choice question

Title: Chapter 01 Question 35

35) The combustion of glucose in oxygen at 298 K is given by the following thermochemical equation:

C₆H₁₂O₆ (s) + 6O₂ → 6CO₂ (g) + 6H₂O (l) = -2808 kJ mol^-1. How much heat energy (in kJ) is supplied when 275 g of glucose burn in a plentiful supply of air so that combustion is complete?

a. 2808.

Section reference: 1.6

b. 4286.19

Section reference: 1.6

c. 772.20

Section reference: 1.6

d. 772200.

Section reference: 1.6

Type: multiple choice question

Title: Chapter 01 Question 36

36) The combustion of butane in oxygen at 298 K is given by the following thermochemical equation:

2 C₄H₁₀ (g) + 13 O₂ → 8 CO₂ (g) + 10 H₂O (l) = -2878 kJ mol^-1. How much heat energy (in kJ) is supplied when 775 g of butane burn in a plentiful supply of air so that combustion is complete?

a. 38370.

Section reference: 1.6

b. 2878.

Section reference: 1.6

c. 2230.45

Section reference: 1.6

d. 2230450.

Section reference: 1.6

Type: true-false

Title: Chapter 01 Question 37

37) When a chemical bond is broken, energy is required to break the bond. This means the bond breaking process is endothermic.

a. True

Section reference: 1.6

b. False

Section reference: 1.6

Type: matching question

Title: Chapter 01 Question 38

38) Match the description with the state of matter it describes.

Section reference: 1.7

a. A rigid form of matter, it has a shape and occupies a fixed volume (at a particular temperature and pressure). = solid

b. A fluid form of matter, it does not have a fixed shape and will expand to fill the container it is in. = gas

c. A fluid form of matter, it occupies a fixed volume (at a particular temperature and pressure) but does not have a fixed shape. = liquid

Type: matching question

Title: Chapter 01 Question 39

39) Match the transition between two states of matter with the enthalpy change for the process.

Section reference: 1.7

a. Δ_vapH^o = Liquid to gas

b. Δ_freezingH^o = Liquid to solid

c. Δ_{reverse sub}H^o = Gas to solid

d. Δ_fusH^o = Solid to liquid

Type: multiple response question

Title: Chapter 01 Question 40

40) Which of the following phase changes are endothermic processes Please select all that apply.

Section reference: 1.7

a. Fusion.

b. Sublimation.

c. Freezing.

d. Reverse sublimation.

Type: matching question

Title: Chapter 01 Question 41

41) Match the non-covalent interaction with an example of a molecule pair that the non-covalent interaction acts between.

Section reference: 1.8

a. London dispersion = C₂H₆, C₄H₁₀

b. Dipole-dipole = CHCl₃, CH₃OH

c. Ion-dipole = Na⁺ and H₂O

d. Hydrogen bond = CH₃OH, H₂O

Type: fill-in-blank

Title: Chapter 01 Question 42

42) London dispersion interactions arise because of the instantaneous ______ that can exist due to the uneven electron distribution within a molecule at a particular instant. This induces a dipole in an adjacent molecule.

Section reference: 1.8

a. dipole

Type: multiple response question

Title: Chapter 01 Question 43

43) Which of the following will alter the position of equilibrium of a reaction in dynamic equilibrium? Please select all that apply.

Section reference: 1.9

a. Pressure of reacting gases.

b. Temperature of reacting solution.

c. Concentration of reacting substances in solution.

d. Time.

Type: true-false

Title: Chapter 01 Question 44

44) Increasing the temperature of an endothermic reaction in dynamic equilibrium will favour the reactants.

a. True

Section reference: 1.9

b. False

Section reference: 1.9

Type: multiple choice question

Title: Chapter 01 Question 45

45) H₂ (g) + I₂ (g) 2HI (g) Construct an expression for the equilibrium constant K_p in terms of partial pressures of the reactant and product gases.

a.

Section reference: 1.9

b.

Section reference: 1.9

c.

Section reference: 1.9

d.

Section reference: 1.9