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Chemistry > C6 - Chemical Synthesis > Flashcards

C6 - Chemical Synthesis Flashcards

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1
Q

What are the uses of chemical synthesis? (6)

A
  • Food additives
  • Fertilisers
  • Dyes
  • Paints
  • Pigments
  • Medicines
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2
Q

What are the 7 steps of chemical synthesis?

A
  1. Choose the reactants and the reaction that will make the substance
  2. Carry out a risk assessment
  3. Work out the quantities needed of reactants
  4. Carry out the reaction in the right conditions to get the best yield quickly and cheaply
  5. Separate the product from the reaction mixture
  6. Purify the product
  7. Check the purity and measure the yield of the product
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3
Q

Relative formula mass

A

The sum of the atomic masses of the atoms in the formula

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4
Q

Actual yield

A

The mass of product measured at the end of the experiment

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5
Q

Theoretical yield

A

How much product should be made based on masses

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6
Q

How is the percentage yield calculated?

A

%yield = actual yield/ theoretical yield x100

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7
Q

What can cause the actual yield to vary? (3)

A
  • Some reactants may remain unreacted
  • Some of the product may be lost when transferring to new containers
  • Some reactants may form other products
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8
Q

Titration

A

A neutralisation reaction used to check purity

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9
Q

What are the steps of titration? (6)

A
  1. If the sample is solid, weigh then dissolve to make a volume of solution
  2. Use a pipette to measure a volume of solution. Use a pipette filler to draw solution into the pipette and empty into a conical flask
  3. Add a few drops of indicator
  4. Place the chemical with the know volume in a burette
  5. Dropped the chemical from the burette into the flask, swirling to mix and reducing the flow to drops close to the endpoint. A colour change marks the end
  6. Note the volume of solution added from the burette as a rough titre then repeat for three close together results or to calculate a mean
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10
Q

Range

A

The spread of readings from highest to lowest

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11
Q

True value

A

A similar value to the mean which is found in the range of very accurate results

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12
Q

Outlier

A

A very different result which may be left out to remove errors in measurement

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13
Q

Rate of reaction

A

The amount of product produced in s certain amount of time

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14
Q

Give an example of a slow and a fast reaction

A

Slow - rusting

Fast - explosion

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15
Q

How is rate of reaction calculated?

A

Change in quantity measured / time taken for change

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16
Q

How is a change in quantity measured if a gas is given off? (2)

A
  • measured the volume of gas at set times using a gas syringe
  • measured the mass lost in he reaction using scales
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17
Q

How is change in quantity measured if a solid is produced? (2)

A
  • measure the time taken for a black cross to disappear under the flask OR
  • use a colorimeter to measure the intensity of the light passing through the flask
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18
Q

Catalyst

A

A substance that speeds up a chemical reaction but is not used up in the process

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19
Q

How can the rate of reaction be increased? (4)

A
  • increasing the temperature
  • increasing the concentration of dissolved reactant
  • breaking solid reactants into pieces to increase their surface area
  • using a catalyst
20
Q

Pure substance

A

A substance that has nothing else mixed with it

21
Q

How do you filter to get a soluble product? (3)

A
  1. Filter out any solid impurities
  2. Evaporate any liquid
  3. Collect the steam and drop into a beaker
22
Q

How do you filter to get an insoluble product? (2)

A
  1. Pour the substance through a filter into a beaker

2. Dry the product left in the filter

23
Q

What are the 5 steps of crystallisation?

A
  1. Dissolve the product in a small amount of hot water, using the minimum needed to dissolve it
  2. Filter off any solid impurities
  3. The filtrate starts to crystallise and some water evaporates off
  4. Filter off the crystals, leaving solid impurities in the solution
  5. Dry the crystals in a desiccator or oven
24
Q

How is a pH meter calibrated

A

By dipping it in a known pH of solution, washing it, then dipping it in the test solution

25
Q

Name two solid acids:

A

Citric and tartaric acid

26
Q

Name three liquid acids:

A

Nitric, sulphuric, ethanoic

27
Q

What substance become hydrochloric acid when dissolved in solution?

A

Hydrogen chloride gas

28
Q

Acid + metal -> ?

A

Salt + hydrogen

29
Q

Acid + metal oxide -> ?

A

Salt + water

30
Q

Acid + metal hydroxide -> ?

A

Salt + water

31
Q

Acid + metal carbonate -> ?

A

Salt + water + carbon dioxide

32
Q

How do you test for hydrogen?

A

Use a lit splint to burn the gas, hydrogen pops

33
Q

How do you test for carbon dioxide?

A

Bubble the gas through limewater, carbon dioxide makes it turn milky

34
Q

What is the formula of sulphuric acid?

A

H2SO4

35
Q

What is the formula of nitric acid?

A

HNO3

36
Q

What is the formula of phosphoric acid?

A

H3PO4

37
Q

What is the charge of a phosphate ion?

A

3-

38
Q

What is the charge of a sulphate ion?

A

2-

39
Q

What is the charge of a nitrate ion?

A

1-

40
Q

What ions are present in acids?

A

Hydrogen H+ ions

41
Q

What ions are present in alkalis?

A

Hydroxide OH- ions

42
Q

What is the ionic state symbol equation for neutralisation?

A

H+(aq) + OH-(aq) -> H2O(l)

43
Q

What is an Exothermic reaction? Give two examples

A

A reaction which gives out heat energy and feel hot e.g. Burning, neutralisation, reaction of water + calcium oxide

44
Q

What is an Endothermic reaction? Give 2 examples

A

Endothermic reactions take in heat from their surroundings so feel cold e.g. Electrolysis or Thermal decomposition

45
Q

Why can Exothermic reactions cause issues in industry if not controlled?

A

They can get out of hand and cause explosions, fires and overheating of equipment

46
Q

Chemical synthesis

A

Using simple substances to make new, useful chemical compounds

Chemistry (6 decks)

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