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Chemistry: Paper 1 > Separate chemistry > Flashcards

Separate chemistry Flashcards

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1
Q

What are the properties of transition metals

A
  • High melting point due to electrostatic forces between positive metal ions and sea of electrons
  • High density
  • Form coloured compounds
  • Useful as catalysts
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2
Q

What causes corrosion

A

Water and oxygen

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3
Q

How does sacrificial protection prevent the rusting of metal

A

Using a more reactive metal to coat a less reactive metal causing it to corrode instead

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4
Q

How can water and oxygen be excluded (not able to affect) from a metal

A
  • Painting
  • Coating with plastic
  • Using oil or grease
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5
Q

How does electroplating improve the appearance and/or the resistance to corrosion of metal objects

A
  • Acts as a barrier to exclude oxygen and water
  • Improves appearance if electroplating with an unreactive metal
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6
Q

Why does converting pure metals into alloys increase the strength of the product

A

Pure metals = have positive ions the same size and in a regular arrangement so layers easily side over each other
Alloy = have positive ions of different metals which have different sized ions so layers can’t slide as easily

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7
Q

Why is iron alloyed with other metals to produce alloy steels

A

So they can be designed to fit a specific use

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8
Q

What are low-carbon steels used for and why

A

Sheeting as they are malleable and easily shaped

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9
Q

What are high carbon steels used for and why

A

Cutting tools since they are hard

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10
Q

What is the alloy of chromium and nickel used for and why

A

Stainless steels (used for cutlery) as they are resistant to corrosion

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11
Q

How is aluminium useful for its property

A

has a low density therefore used for aircraft

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12
Q

How is copper useful for its property

A

Good electrical conductor therefore used in cables

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13
Q

How is gold useful for its property

A

Good resistance to corrosion therefore used in jewlery

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14
Q

How is magnalium (aluminium + magnesium) useful for its property

A

Low density therefore good for cars and planes

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15
Q

How is Brass (copper + zinc) useful for its property

A

Hard and resistant to corrosion therefore used in coins

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16
Q

How do you work out concentration of a solution (2 ways)

A
  • concentration (g/dm^3) = mass (g) ÷ volume (dm^3)
  • concentration (mol dm^-3) = number of moles ÷ volume of solution (dm^3)
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17
Q

What are the two ways of showing concentration

A

g/dm3 or mol/dm3

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18
Q

How do you convert g/dm3 to mol/dm3

A

divide by the relative formula mass/molar mass

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19
Q

How do you convert from mol/dm3 to g/dm3

A

multiply by the relative formula mass

20
Q

How do you convert a cubic centimetre into a cubic decimetre

A

divide by 1000

21
Q

How do you convert a cubic decimetre into a cubic centimetre

A

multiply by 1000

22
Q

How do you carry out an acid-alkaline practical

A
  • add acid to burette using a funnel, record the volume in the burette to
    start
  • add known volume of alkali to a conical flask and add some indicator
  • place conical flask on white tile (so you can see colour change clearly)
  • add acid to alkali and swirl until you reach the end point
  • calculate how much acid has been added (titre)
  • repeat until you get concordant titres
23
Q

How do you work out percentage yield

A

(actual yield / theoretical yield) x 100

24
Q

What are some causes for the actual yield being smaller than theoretical yield

A
  • incomplete reactions
  • side reactions
  • reversibile reaction
25
Q

What is atom economy

A

Amount of useful products gained from the reactances

26
Q

How do you work out atom economy

A

atom economy = (Mr of desired product from reaction / sum of Mr of all reactants) x 100

27
Q

Explain why a particular reaction pathway is chosen to produce a specified product

A

To produce a:
* a high atom economy
* a high yield
* at faster rate

28
Q

What is molar volume in cm^3 and dm^3)

A

cm^3 = 24,000
dm^3 = 24

29
Q

How do you calculate the volume of a gas

A

Volume = amount in mol × molar volume

30
Q

What is Avogadro’s law

A

One mole of a substance contains 6.02 x 10^23 particles

31
Q

How is equilibrium achieved at a faster rate

A
  • Higher temperature is used
  • A higher pressure
  • A higher concentration is used
  • A catalyst is used
32
Q

How does temperature affect equilibrium

A

Increase of temperature: equilibrium will shift to favour the reaction which will reduce the temperature. (endothermic)

Decrease of temperature: equilibrium will shift to favour the reaction which will increase the temperature. (exothermic)

33
Q

How does pressure affect equilibrium

A

Increase of pressure: reaction favours the side with a smaller molar volume

Decrease of pressure: reaction favours the side with a larger molar volume

34
Q

What 3 compounds are used in fertilisers to increase agriculture

A
  • Nitrogen
  • Phosphorus
  • Potassium
35
Q

How does ammonia react with nitric acid to produce a salt that is
used as a fertiliser

A

ammonia + nitric acid → ammonium nitrate
(NH3 + HNO3 → NH4NO3)

36
Q

What is the equation for forming ammonium nitrate

A

(NH3 + HNO3 → NH4NO3)

37
Q

Describe the process of making ammonia sulphate in a lab

A
  • reactants: ammonia solution and dilute sulfuric acid (bought from
    chemical manufacturers)
  • SMALL scale
  • only involves a few stages (titration then crystallisation)
38
Q

Describe the process of making ammonia sulphate in an industry

A
  • Ammonia: natural gas, air, water
  • Sulfuric acid: sulphur, air,
    water
  • LARGE scale
    ○ Many stages required (need to make ammonia and sulfuric acid, react
    accurate volumes then evaporate)
39
Q

How does a catalyst affect equilibrium

A
  • doesn’t shift the position of equilibrium
  • allows the equilibrium to be established faster
  • less heat is needed
40
Q

what happens if you increase the concentration of a reactant?

A

increasing the concentration of a reactant system makes more products to balance it out

41
Q

NA

A

NA

42
Q

When do chemical reactions stop

A

Chemical reactions stop when one of the reactants has been used up

43
Q

What is the reaction in a hydrogen fuel cell

A

Hydrogen + Oxygen → Water
2H2 + O2 → 2H2O

44
Q

What are the positives of using fuel cells

A
  • produce only water as a waste
  • Keeps producing fuel if being supplied
45
Q

What are the negatives of using fuel cells

A
  • difficult to transport/store hydrogen so
    aren’t suitable for portable devices
  • expensive to make

Chemistry: Paper 1 (5 decks)

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