Deck 1: Fundamentals

Question 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.

Answer 1

seven

Question 2

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

A) 1.275 × 10^-12 m.
B) 1.275 Å.
C) 0.1275 nm.
D) 1.275 × 10^-10 mm.

Answer 2

B, C

Question 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.
-100 °C

A) 373.15 K
B) 273.15 K
C) 0 K
D) 298 K

Answer 3

A

Question 4

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.
-0 °C

A) 373.15 K
B) 273.15 K
C) 0 K
D) 298 K

Question 5

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.
--273.15 °C

A) 373.15 K
B) 273.15 K
C) 0 K
D) 298 K

Question 6

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.
-25 °C

A) 373.15 K
B) 273.15 K
C) 0 K
D) 298 K

Question 7

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

A) atm.
B) Kg m^-1 s^-2.
C) bar.
D) g mm^-1 s^-2.

Question 8

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

A) The same number of protons.
B) The same number of neutrons.
C) A different number of electrons.
D) A different number of neutrons.

Question 9

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

A) 18.
B) 36.
C) 22.
D) 40.

Question 10

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

Question 11

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

Question 12

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

A) 12 g.
B) 0.045 g.
C) 1753.033 g.
D) 6.022 × 10²³ g.

Question 13

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

A) 0.26 mol.
B) 3.86 mol.
C) 13939.49 mol.
D) 5.26 mol.

Question 14

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 ______.

Question 15

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

Question 16

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.

A) W = 2.
B) X = 6.
C) Y = 6.
D) Z = 6.

Question 17

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.
B) 578 g.
C) 384 g.
D) 500 g.

Question 18

What is the oxidation state of C in Li₂CO₃?

A) +1.
B) +2.
C) +3.
D) +4.

Question 19

What is the oxidation state of N in KNO₂?

A) +1.
B) +2.
C) +3.
D) +4.

Question 20

In the reaction of lithium with water lithium has been ________.
2 Li(s) + 2 H₂O(l) → 2 LiOH(aq) + H₂(g)

Question 21

The systematic name for SF₆ is sulphur ____fluoride

Question 22

Match the following brief description with the correct term:
-involves the transfer of a proton

A) Acid-base reaction
B) Precipitation reaction
C) Redox reaction
D) Complexation reaction

Question 23

Match the following brief description with the correct term:
-involves the formation of a solid product when two solutions are mixed

A) Acid-base reaction
B) Precipitation reaction
C) Redox reaction
D) Complexation reaction

Question 24

Match the following brief description with the correct term:
-involves the formation of a complex

A) Acid-base reaction
B) Precipitation reaction
C) Redox reaction
D) Complexation reaction

Question 25

The systematic name for XeF₄ is xenon _____fluoride

Question 26

The systematic name for SiO₂ is silicon __oxide

Question 27

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.
B) -2.
C) 0.
D) +1.

Question 28

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
B) 0.57
C) 95
D) 0.095

Question 29

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.
B) 74550 g.
C) 149.10 g.
D) 74.55 g.

Question 30

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

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.

Question 31

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.
B) 401241 g.
C) 1.875 g.
D) 535 g.

Question 32

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 .
B) 0.134
C) 0.0875
D) 2.45

Question 33

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
B) 3.7 × 10^-3.
C) 0.296
D) 0.148

Question 34

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.
B) 0.031
C) 3.10 × 10^-5.
D) 0.073

Question 35

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
B) 0.28
C) 0.25
D) 7.0875 × 10^-3

Question 36

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

Question 37

An exothermic reaction has a ________ enthalpy change.

Question 38

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

Question 39

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

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.

Question 40

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.
B) 4286.19
C) 772.20
D) 772200.

Question 41

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.
B) 2878.
C) 2230.45
D) 2230450.

Question 42

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

Question 43

Match the description with the state of matter it describes.
-A rigid form of matter, it has a shape and occupies a fixed volume (at a particular temperature and pressure).

A) solid
B) gas
C) liquid

Question 44

Match the description with the state of matter it describes.
-A fluid form of matter, it does not have a fixed shape and will expand to fill the container it is in.

A) solid
B) gas
C) liquid

Question 45

Match the description with the state of matter it describes.
-A fluid form of matter, it occupies a fixed volume (at a particular temperature and pressure) but does not have a fixed shape.

A) solid
B) gas
C) liquid

Question 46

Match the transition between two states of matter with the enthalpy change for the process.
-Δ_vapH^o

A) Liquid to gas
B) Liquid to solid
C) Gas to solid
D) Solid to liquid

Question 47

Match the transition between two states of matter with the enthalpy change for the process.
-Δ_freezingH^o

A) Liquid to gas
B) Liquid to solid
C) Gas to solid
D) Solid to liquid

Question 48

Match the transition between two states of matter with the enthalpy change for the process.
-Δ_{reverse sub}H^o

A) Liquid to gas
B) Liquid to solid
C) Gas to solid
D) Solid to liquid

Question 49

Match the transition between two states of matter with the enthalpy change for the process.
-Δ_fusH^o

A) Liquid to gas
B) Liquid to solid
C) Gas to solid
D) Solid to liquid

Question 50

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

A) C₂H₆, C₄H₁₀
B) CHCl₃, CH₃OH
C) Na⁺ and H₂O
D) CH₃OH, H₂O

Question 51

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

A) C₂H₆, C₄H₁₀
B) CHCl₃, CH₃OH
C) Na⁺ and H₂O
D) CH₃OH, H₂O

Question 52

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

A) C₂H₆, C₄H₁₀
B) CHCl₃, CH₃OH
C) Na⁺ and H₂O
D) CH₃OH, H₂O

Question 53

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

A) C₂H₆, C₄H₁₀
B) CHCl₃, CH₃OH
C) Na⁺ and H₂O
D) CH₃OH, H₂O

Question 54

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.

Question 55

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

A) Pressure of reacting gases.
B) Temperature of reacting solution.
C) Concentration of reacting substances in solution.
D) Time.

Question 56

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

Question 57

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)

B)

C)

D)