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Chemistry by Thaidz > Chem in industry > Flashcards

Chem in industry Flashcards

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1
Q

what are metal ores ?

A

(reactive metals in the ground that form compounds with other elements)
compounds with enough metal to make worth while to extract

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2
Q

describe the industry reactivity series

A 
potassium 
sodium 
calcium
magnesium
aluminium 
CARBON
zinc
iron
tin
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3
Q

describe electrolysis

A

melt metal for free ions
positive metal electrons go to cathode (-ve)
negative electrons go to anode (+ve)
metal becomes full atom and sinks
oxygen reacts together and carbon and lifts
this is why carbon anode must be replaced
REDOX REACTION

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4
Q

why is electrolysis expensive ?

A

needs lots of electricity
needs to heat electrolyte
disappearing (+ve) electrode needs constant replacement

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5
Q

what is aluminium extracted from ?

A

bauxite (A2 O3)

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6
Q

what is iron extracted from ?

A

haematite (Fe O3)

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7
Q

uses of coke for extraction of iron?

A

almost pure carbon so reduces iron oxide

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8
Q

uses of limestone for extraction of iron?

A

takes away impurities in form of slag

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9
Q

steps for extracting iron :

A

hot air blasted into furnace
coke burns to produce CO2
CO2 reacts with unburnt coke to produce CO
CO reduces iron ore
iron then runs to bottom and is tapped off

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10
Q

describe process of impurities in extracting iron

A

limestone thermally decomposes
calcium oxide reacts with sand
calcium silicate forms (slag) which is tapped off

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11
Q

formula for sand

A

Si O2

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12
Q

uses for slag?

A

road building

fertiliser

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13
Q

uses for wrought iron

A

almost pure iron so used for gates and railings

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14
Q

uses for cast iron

A

iron + carbon + silicon (hard but brittle, used for manhole covers / cooking pans)

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15
Q

uses for steel

A

an alloy of iron, carbon and others
harder than pure iron but still malleable
used for construction and carbodies

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16
Q

uses for stainless steel

A

iron and chromium and doesn’t rust so used for cutlery

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17
Q

uses for aluminium

A

drinks cans (no rust) and aeroplane frames (light metal)

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18
Q

why doesn’t aluminium corrode easily?

A

reacts with oxygen to form a protective aluminium oxide layer

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19
Q

what is crude oil?

A

mixture of hydrocarbons

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20
Q

describe industry fractional distillation

A

oil heated until most is gas
passed through fractionating column with temp gradient
when substances reaches lower than B.P. they condense
bubble caps prevent leakage

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21
Q

during industry fractional distillation, where do long hydrocarbons condense ?

A

high B.P. so at the bottom

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22
Q

during industry fractional distillation, where do short hydrocarbons condense ?

A

low B.P. so at the top

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23
Q

industry factional distillation order ?

A 
refinery gases
gasoline
naphtha
kerosene (paraffin)
diesel
fuel oil
bitumen
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24
Q

uses for refinery gases

A

bottled gas , heating and making glass

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25
Q

uses for gasoline

A

car fuel

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26
Q

uses for naphtha

A

starting material for plastics, dyes, drugs…

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27
Q

uses for kerosene (paraffin)

A

jet fuel, domestic heating and paint

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28
Q

uses for diesel

A

fuel for larger motors

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29
Q

uses for fuel oil

A

fuel for big ships and central heating

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30
Q

uses for bitumen

A

roads and roofs

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31
Q

how is carbon monoxide formed?

what effect does it have?

A

when hydrocarbon fuels burn without enough oxygen (incomplete combustion)
poisonous as stops cells carrying blood

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32
Q

how are sulfur dioxide and nitrogen oxides formed?

what effects does they have?

A

released when fossil fuels burnt :
-SO2 comes from sulfur impurities in fuels
-NO(2)s created when temp high enough for N and O2 to react
cause acid rain

33
Q

what is acid rain caused by ?

what effect does it have?

A

carbon dioxide, sulfur dioxide and nitrogen oxides
makes lakes acidic (kills life)
damages limestone buildings and stone statues

34
Q

why do we need cracking?

A

demand for shorter hydrocarbons is much higher (e.g. petrol) and also produces alkenes (for polymers)

35
Q

what is cracking ?

A

thermally decomposing long hydrocarbons into shorter hydrocarbons + alkenes, sped up with a catalyst

36
Q

describe the cracking process

A

alternate heat between paraffin and catalyst until paraffin vaporizes and catalyst glows red
(the heated paraffin cracks over catalyst)
small alkane collected at end of tube
alkene gas collected in gas jar

37
Q

how are addition polymers made up ?

A

monomers with C=C (alkenes) under high pressure + catalyst makes their bonds open up and they connect up to form long saturated chains

38
Q

conditions for cracking

A

silica or alumina catalyst

600 - 700 degrees Celsius

39
Q

what is condensation polymerization ?

A

reacting 2 different monomers so they bond and form a polymer
for each new bond, a small molecule is lost (e.g. water)

40
Q

uses for poly(ethene)

A

it is light and stretchable so is ideal for packaging (plastic bottles and bags…)

41
Q

uses for poly(propene)

A

it is tough, relatively flexible and heat resistant so used for kettles, food containers …

42
Q

uses for (chloroethene)

A

used for clothes, pipes and insulating electrical wires

43
Q

why are polymers hard to get rid of?

A

they are inert as their C-C bond is very strong so can’t easily be broken
this means it takes long for them to biodegrade so it is best to recycle/reuse

44
Q

what is haber process for ?

A

making ammonia

45
Q

equation for haber process

A

N² (g) + 3H² (g) 2NH³ (g) (+heat)

46
Q

where are nitrogen and hydrogen obtained from for haber process ?

A

nitrogen - air

hydrogen - natural gas / cracking

47
Q

conditions for haber process

A

pressure : 200 atm
temp : 450 degrees Celsius
catalyst : iron

48
Q

describe the pressure in haber process

A

set high (200) to give best % yield (as high pressure favors forward reaction) (4-2)

49
Q

describe the temp in haber process

A

set high even tho it moves the equilibrium the wrong way as making it cold would slow the reaction

50
Q

describe what happens to the reactants in haber process

A

form ammonia which is a gas but cools and liquefies to be collected
unused H and N recycled

51
Q

what does the catalyst do in the haber process ?

A

speeds up the reaction without affecting the % yield

52
Q

uses for ammonia

A

used to make nitric acid
can also make ammonia nitrate (ammonia + nitric acid)
ammonia nitrate used in fertilizers (plants use nitrogen to make proteins)

53
Q

what is contact process for ?

A

making sulfuric acid

54
Q

describe the steps of contact process

A

burn sulfur in air to form sulfur dioxide
oxidize sulfur dioxide (+ catalyst) to form sulfur trioxide
sulfur trioxide dissolved in sulfuric acid to form oleum
oleum dilluted with water to form sulfuric acid

55
Q

describe what is needed for step 2 of contact process

A

increase pressure for best % yield
should reduce temp however slows the reaction so hot
catalyst important !

56
Q

conditions for contact process

A

temp : 450
pressure : 1 or 2
catalyst : vanadium (V) oxide

57
Q

uses for sulfuric acid

A

fertilizers
detergents
paints

58
Q

hydrogen in electrolysis of brine

A

given off at cathode as two H ions accept two electrons to become one H² molecule

59
Q

chlorine in electrolysis of brine

A

given off at anode as two Cl ions lose their electrons to become one Cl² molecule

60
Q

sodium and hydroxide in electrolysis of brine

A

stay in solution (hydroxide from water) and react to form sodium hydroxide

61
Q

how to test if a liquid is an electrolyte?

A

place conductivity probe into and look at reading

or set up electrolytic cell and see if electrolysis undergoes

62
Q

what is different with electrolysis in aqueous solutions?

A

hydrogen and hydroxide ions are present

63
Q

what happens at the cathode in aqueous electrolysis?

A

if metal more reactive than H+ ions, hydrogen gas produced

if metal less reactive, layer of pure metal produced

64
Q

what happens at the anode in aqueous electrolysis?

A

if OH- and halide ions present, molecules of Cl², Br² and I² form
if no halide ions, oxygen forms

65
Q

how to increase amount of product in electrolysis ?

A

increase no. of electrons by:
electrolise for longer
increase the current

66
Q

charge =

A

current x time

67
Q

what is one Faraday ?

A

one mole of electrons

68
Q

what are the two ways of making ethanol?

A

reacting ethene and steam

fermentation

69
Q

How can you make ethanol from ethene?

what are the advantages / disadvantages ?

A

react with steam
cheap process and not much is wasted
non-renewable so will run out/become expensive

70
Q

conditions for ethene + steam

A

300 degrees 60-70 atm phosphoric acid catalyst

71
Q

How can you make ethanol from fermentation?

what conditions?

A 
convert sugar (e.g. glucose) into ethanol using yeast 
30 degrees
72
Q

what are the advantages / disadvantages of fermentation to produce ethanol ?

A

renewable therefore reliable

not very concentrated therefore must be purified and distilled

73
Q

describe the dehydration of ethanol

A

remove water from ethanol to form ethene by soaking ceramic wool with it and heat next to aluminium oxide catalyst
as vapour passes over hot catalyst, it becomes ethene gas

74
Q

When at cathode, ions are always…

A

Reduced (gain of electrons)

75
Q

When at anode, ions always…

A

Oxidised (loss of electrons)

76
Q

What is an electrolyte ?

A

Substance that contains ions and undergoes electrolysis

77
Q

Coulomb =

A

Time (s) x amps

78
Q

1 mile of coulombs =

A

96000 coulombs (1 faraday)

79
Q

What is cryolite for?

A

Used to dissolve aluminium oxide to lower (keep temp low)

Chemistry by Thaidz (5 decks)

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