DEVELOPING FUELS

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84 Terms

1
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What volume does 1 mole of gas always occupy at room temperature and pressure?

24.0dm³ (or 24000cm³)

2
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What happens to temperature in exothermic reactions?

Increases

3
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On an enthalpy level diagram, if something is high then whats its stability?

The higher something is the less stable

4
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What is enthalpy? (in the most simple terms)

Stored heat energy

5
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What are the units for enthalpy change?

KJmol-1

6
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What is the ideal gas equation?

pV = nRT

7
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Standard enthalpy change of combustion=

Enthalpy change when 1 mole of a substance is completely combusted under standard condition

8
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Standard enthalpy change of formation=

Enthalpy change when 1 mole of a substance is formed from its elements under standard condition

9
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Standard enthalpy change of neutralisation=

Enthalpy change when 1 mole of H2O is formed when an acid and alkali react under standard condition

10
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Standard enthalpy change of reaction=

The enthalpy change when the reaction occurs in molar quantities shown in the chemical equation, under standard condition.

11
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Why is the enthalpy change in standard conditions?

It allows for comparison

12
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What are the standard conditions?

298K / 100kPa / 1moldm^-3

13
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Breaking bonds are…

Endothermic

14
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Forming bonds are…

Exothermic

15
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What is enthalpy change?

The heat energy transferred in a reaction at constant pressure (kJmol^-1)

16
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Unit of pressure in the ideal gas equation

Pa

17
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Unit of volume in the ideal gas equation

18
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Unit of temperature in the ideal gas equation

K / kelvin

19
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What is ‘R‘ in the ideal gas equation?

Gas constant

20
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3 ways of finding enthalpy change of reaction

Doing experiments / use Hess cycles / use bond enthalpy values

21
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Does forming bonds make them become more or less stable?

More stable

22
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What are the 2 main procedural problems of enthalpy change of combustion experiments?

Heat loss to surrounding / Incomplete combustion

23
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What is the Hess’s law?

The enthalpy change is independent of the path taken

24
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Why would a reaction be endothermic?

The E needed to break bonds is more than the E released from forming bonds

25
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Describe an experiment they could use to determine the enthalpy change of combustion of liquid hexane in the laboratory (1 mark)

Burn the (known mass of) fuel under a container of (known volume of) water and measure the temperature increase of H2O

26
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6 Ways to make basic experiment more accurate:

Use a lid / Use draught shield / Move calorimeter closer to flame / Use a bomb calorimeter / Stir to improve heat distribution / Use copper calorimeter instead of beaker

27
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What is the empirical formula?

Simplest ratio of atoms in a molecule

28
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What is the molecular formula?

Actual number of each type of atom in a molecule

29
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A property of the molecular formula

No information about structure (ie don‘t show functional group)

30
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What is the general formula?

Describes all member of a homologous series

31
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Aliphatic

Does not contain a benzene ring

32
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Aromatic

Contains a benzene ring

33
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Arene

Contains a benzene ring

34
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What is the functional group?

The part which reacts

35
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All the bond angles (/shape) in saturated hydrocarbons are…

109.5 / tetrahedral

36
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What are the 3 reactions alkanes can do?

Combustion / radical substitution with halogen / Cracking

37
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What is the reason for cracking alkanes?

Long hydrocarbons are not useful, so we have to convert them into shorter, more useful products

38
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What are the 2 types of cracking (in industry)?

Catalytic cracking / Steam cracking

39
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Conditions for catalytic cracking in industry

500 degrees Celsius / zeolite catalyst

40
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<p>What is this practical?</p>

What is this practical?

Cracking in the lab

41
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What is a catalyst?

Provides an alternative pathway with a lower Ea. Chemically unchanged at the end of the reaction.

42
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What are homogeneous catalysts?

Catalysts and reactants are in the same state

43
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What are heterogeneous catalysts?

Catalysts and reactants are in different states

44
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Step 1 of heterogeneous catalysts reaction

The reactant molecules are adsorbed onto the catalyst surface weakening bonds within the reactants

45
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Step 2 of heterogeneous catalysts reaction

Bonds within the reactant molecules break

46
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Step 3 of heterogeneous catalysts reaction

New bonds form, making the product molecules

47
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Step 4 of heterogeneous catalysts reaction

The product molecules leave the catalyst surface (desorption)

48
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Write the chemical equation that happens in the catalytic converters in cars.

CO + NO —> CO2 + 1/2N2

49
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How is CO formed in cars are why is it bad?

Incomplete combustion / its toxic

50
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How is NO formed in cars are why is it bad?

N2 and O2 form the air react due to high temperature / respiratory irritant, causes photochemical smog and causes acid rain

51
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(3) What elements are used as catalyst in cars

Pt / Rh / Pd

52
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How can a catalyst be poisoned?

When other reactants adsorb strongly onto the surface and don’t react, blocking the surface and stopping the normal reactants from adsorbing.

53
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What does ‘Adsorbed’ mean (in catalytic converters)

Form weak bonds with the surface (catalytic surface)

54
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What are structural isomers?

Structural isomers have the same molecular formula but different structural formula

55
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What are stereoisomers?

Stereoisomers have the same structural formula but different arrangement of atoms in space

56
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What are the 2 criteria‘s for stereoisomerism (E/Z)

There must be a C=C as this restricts rotation / There must be 2 different groups on each C of the C=C

57
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What are the 2 electrophilic addition reactions of alkenes with halogens?

Alkenes + X2 —> Dihaloalkane / Alkenes + HX —> Haloalkane

58
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What are the 2 electrophilic addition reactions of alkenes without halogens?

Alkene + H2 —> Alkane / Alkene + H-OH —> Alcohol

59
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What are the conditions for [Alkenes + X2 —> Dihaloalkane]

RTP

60
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What are the conditions for [Alkenes + HX —> Haloalkane]

RTP

61
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What are the conditions for [Alkene + H2 —> Alkane]

Nickle catalyst + high T&P / Platinum catalyst + RTP

62
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What are the conditions for [Alkene + H-OH —> Alcohol]

H2PO4 catalyst + high T&P / conc. H2SO4 + steam

63
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64
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65
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What are curly arrows for?

Curly arrows show the movement of e-

66
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Where can curly arrows start? (2)

From a lone pair / from the middle of a bond

67
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<p>What is this?</p>

What is this?

Mechanism for propene reacting with Cl2

68
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What is an electrophile?

A positive or partially positive species which forms a dative bond by accepting a pair of electrons

69
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Test for proof for mechanism? (of ethene with bromine)

Add a solution of NaCl, only forms dibromoethane OR 1-bromo2-chloroethane (NEVER dichloroethane).

70
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What does ‘sharing of pairs of electrons‘ suggest about the orbitals?

The orbitals are overlapping

71
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What are the 2 types of overlap (of orbitals)?

End on overlap along the internuclear axis (sigma) / Sideways overlap of 2 parallel p orbitals above and below the internuclear axis (Pi)

72
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A double bond is…

One sigma bond + One Pi bond

73
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A triple bond is…

One sigma bond + Two Pi bonds

74
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Source for CO2

Complete combustion of fossil fuels

75
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Source for CO

Incomplete combustion of fossil fuels

76
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Source for NO / NO2

N2 and O2 from the air react due to high temperatures in engine

77
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Source for SO2

From S impurities in fuels

78
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Source for N2O4

Ploughing fertilized fields

79
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Why is SO2 a problem?

Causes acid rain (H2SO4)

80
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Why is N2O4 a problem?

Respiratory irritant

81
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Example for biofuel (/how its made)

Ethanol, which can be made from plants, by fermentation of their sugars. It is usually mixed with petrol

82
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Advantages for biofuels (4)

Helps car engine perform well / carbon neutral / renewable / produces less CO

83
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Disadvantages of biofuels

Needs a lot of land to grow the crops, which could otherwise be used to grow food / a lot of energy is needed for intensive cultivation of the crop

84
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Shape and bond angles of alkanes

Tetrahedral, 109.5