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Chemistry exam questions > Mock 2008 > Flashcards

Mock 2008 Flashcards

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1
Q

Explain what is meant by a primary standard solution?

A

A substance that is available in 100% purity, is stable in air, has a high molar mass for accuracy and dissolves easily in water and can be made up to a standard solution directly.

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2
Q

Why is potassium manganate (VII) not considered to be a primary standard?

A

xx

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3
Q

Why was sulphuric acid added to the conical flask?

A

x

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4
Q

Name the piece of equipment that should be used to transfer the 25 cm3 of ammonium iron (II) sulphate to the conical fl ask.

A

x

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5
Q

Describe the correct procedure for rinsing this piece ^^ of equipment and transferring the solution to the conical flask.

A

x

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6
Q

In an experiment the primary standard ammonium iron (II) sulphate was used to standardise a solution of potassium manganate (VII). What colour change would you observe as the solution from the burette flows into the conical flask and how was the end point detected?

A

x

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7
Q

In an experiment the primary standard ammonium iron (II) sulphate was used to standardise a solution of potassium manganate (VII). What is the role of the Mn2+ ions produced in this reaction?

A

x

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8
Q

Describe the appearance of the solid Y ^&^&

A

x

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9
Q

Write a balanced equation for the reaction between && and &&* producing ethyne.

A

x

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10
Q

Name two impurities found in the ethyne gas produced and say how these impurities may be removed.

A

x

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11
Q

Ethyne, C₂H₂, is described as an unsaturated hydrocarbon. What is meant by the term unsaturated?

A

A multiple bond present between two carbon atoms.

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12
Q

Name the reagent used to test for unsaturation and state the type of reaction involved.

A

x

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13
Q

What is the common name for ethyne and state one major use of the gas?

A

h

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14
Q

In which of the two solvents water or methylbenzene is ethyne soluble? Explain why.

A

n

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15
Q

Write a balanced equation for the decomposition of hydrogen peroxide.

A

d

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16
Q

State Charles Law.

A

At a constant pressure, the volume of a fixed mass of any gas is directly proportional to the absolute temperature. (Kelvin)

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17
Q

Define reduction in terms of electron transfer.

A

Reduction is the gain of electrons.

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18
Q

How could you test for the presence of the nitrate ion in aqueous solution?

A

x

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19
Q

Atomic Absorption Spectrometry is used to detect heavy metals e.g. lead in water. What is the underlying principle in this analytical technique.

A

xx

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20
Q

Account for the trend in the size of the atomic radius going across a period in the periodic table.

A

xx

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21
Q

How many atoms are present in 560 cm³ of ammonia at s.t.p.

A

x

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22
Q

Give the systematic name of the compound

CH₃C(CH₃)₂CH₂CH(CH₃)CH₃.

A

x

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23
Q

What are alpha particles?

A

x

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24
Q

Write the (i) conjugate acid and (ii) the conjugate base of HSO₄-.

A

xx

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25
Q

How does nitrogen fixation occur in nature?

A

x

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26
Q

Give an example of (i) an ionic crystal and (ii) a covalent macromolecular crystal.

A

xx

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27
Q

Define first ionization energy.

A

x

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28
Q

Account fully for the trends in first ionisation energies of elements across the second period of the periodic table (i.e. Li to Ne).

A

x

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29
Q

Account for the trend in first ionisation energies of the elements going down Group II of the periodic table, i.e. the alkaline-earth metals.

A

x

30
Q

What contribution did Dobereiner make to the systematic arrangement of the elements?

A

x

31
Q

State two ways in which Mendeleev’s periodic table of elements differs from that of Moseley.

A

x

32
Q

Define relative atomic mass.

A

x

33
Q

Calculate the relative atomic mass of chlorine given the following isotopic composition: chlorine-35 = 75% and chlorine-37 = 25%.

A

x

34
Q

Define heat of reaction.

A

x

35
Q

The combustion of 2,2,4-trimethylpentane may be described by the following balanced equation: 2C8H18(l) + 25O2(g) 16CO2(g) + 18H2O(l)
Given that the heats of formation of 2,2,4-trimethylpentane, carbon dioxide and water are –259, –394 and –286 kJ mol–1, respectively, calculate the heat of combustion of 2,2,4-trimethylpentane.

A

x

36
Q

What is the octane number of a fuel?

A

x

37
Q

The organic compound 2,2,4-trimethylpentane is one of the reference hydrocarbons used in measuring the octane number of a fuel. Name the other reference hydrocarbon.

A

x

38
Q

What structural feature of 2,2,4-trimethylpentane gives it such a high octane number. Give one other structural feature which increases the octane rating of a hydrocarbon.

A

x

39
Q

There are two structural isomers of the hydrocarbon of formula C4H8. In the case of each of these isomers, draw the structure of the molecule and give its systematic IUPAC name.

A

x

40
Q

Name the compound: C₂H₄

A

x

41
Q

Name the compound: C₂H₅OH

A

x

42
Q

Name the compound: C₂H₅ONa

A

x

43
Q

Name the compound: C₂H₅COOC₂H₅

A

x

44
Q

Identify the type of reaction represented by the letters X and Z.
X
C₂H₄ → C₂H₅OH → C₂H₅ONa
Z ↳ C₂H₅COOC₂H₅

A

x

45
Q

Draw C₂H₅COOC₂H₅ and indicate on the diagram a carbon atom which has a planar geometry and a carbon atom which has a tetrahedral geometry.

A

x

46
Q

Name the reactant added to C₂H₅OH in order to form the compound C₂H₅COOC₂H₅.
C₂H₄ → C₂H₅OH → C₂H₅ONa
↳ C₂H₅COOC₂H₅

A

x

47
Q

The compound C₂H₄ reacts with hydrochloric acid to form C₂H₅Cl. Describe the mechanism of the reaction involved in this conversion.

A

x

48
Q

Distinguish between the primary and secondary stages of sewage treatment.

A

zx

49
Q

Sewage treatments plants may also carry out a tertiary process which reduces the levels of certain substances. Name these substances and explain why their removal is necessary.

A

x

50
Q

In the treatment of water for drinking, aluminium sulphate is added. State the purpose of this addition and name the process involved.

A

x

51
Q

Explain how an acid-base indicator XOH which is itself a weak base functions.

A

x

52
Q

Calculate the pH of a 0.2M ammonia (NH₃) solution given that the dissociation constant Kb for ammonia is 1.8 ¯ 10-5. What is the pH of a sodium hydroxide (NaOH) solution of the same concentration.

A

x

53
Q

State Le Chátelier’s principle.

A

x

54
Q

question 9 is missing do it on a page

A

x

55
Q

Write out the electronic configuration (s, p, etc.) of a neutral chromium atom.

A

x

56
Q

Describe using a dot and cross diagram the bonding in the ammonia molecule.

A

x

57
Q

What is the shape of the ammonia molecule?

A

x

58
Q

Which of the following angles 1070, 1090, and 1110 would you expect to be closest to the bond angle found in the ammonia molecule?

A

x

59
Q

What is a catalyst?

A

x

60
Q

Name the two theories of catalysis. State which of these theories occur in the catalytic converter in a car.

A

x

61
Q

Name one element used as a catalyst in a catalytic converter. State and explain the effect leaded petrol has on a catalytic converter.

A

x

62
Q

Ethanal is prepared in the laboratory according to the following equation: 3C₂H₅OH + Cr₂O72– + 8H+ 3CH₃CHO + 2Cr³+ + 7H₂O If 7.4g of sodium dichromate (Na2Cr2O7.2H2O) and 5.6g of ethanol (C2H5OH) are used in the reaction determine which of the two reagents are present in excess. After purification 1.2g of ethanal was obtained, calculate the percentage yield. (12) [Relative atomic masses: Na = 23: Cr =52: O =16: H = 1 C = 12: ]

A

x

63
Q

Describe a test which could be carried out to identify the presence of the phosphate ion in aqueous solution.

A

x

64
Q

What test could be carried out to distinguish between the two phosphate salts copper phosphate (Cu₃(PO₄)₂) and sodium phosphate (Na₃PO₄)? What observation would be made in this test?

A

x

65
Q

Explain the term electrolysis.

A

x

66
Q

A solution of sodium sulphate was electrolysed using the following apparatus. Write the balanced half equations for the reactions that occur at the anode and the cathode. If universal indicator is added to the solution at the start of the experiment describe the colour change that occurs at each electrode.

A

x

67
Q

What is the approximate percentage of (i) nitrogen and (ii) oxygen in air?

A

x

68
Q

Explain how oxygen and nitrogen are produced for industrial use.

A

x

69
Q

State any two uses of (i) nitrogen gas and (ii) oxygen gas.

A

x

70
Q

What is corrosion? Explain in terms of electron transfer what occurs when iron corrodes.

A

x

71
Q

Name two substances that accelerate the corrosion of iron. Give a reason for each.

A

x

72
Q

Name one method that may be used to prevent the corrosion of iron.

A

x

Chemistry exam questions (29 decks)

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