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Higher Chemistry > Chemistry in society- Unit 3 > Flashcards

Chemistry in society- Unit 3 Flashcards

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1
Q

Haber process equation

A

N2 + H2 = NH3

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2
Q

Ostwald process equation

A

NH3+H2O+O2=HNO3

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3
Q

Catalyst used in haber process

A

Iron

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4
Q

Catalyst used In Ostwald process

A

Platinum

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5
Q

The haber process uses

A

Gases from the atmosphere

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6
Q

Before you can do the Ostwald process what needs to happen first

A

The haber process

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7
Q

What is fractional distillation

A

The seperation of crude oil into fractions according to their boiling points

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8
Q

How many stages is there when manufacturing chemicals

A

4

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9
Q

Stage 1 of manufacturing chemicals

A

Research and development

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10
Q

Stage 2 of manufacturing chemicals

A

Laboratory process

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11
Q

Stage 3 of manufacturing chemicals

A

Pilot plant

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12
Q

Stage 4 of manufacturing chemicals

A

Production plant- final stage

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13
Q

How many principles are in the design process

A

7

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14
Q

Stage 1 of design process

A

Availablity Of feedstock

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15
Q

Stage 2 of design process

A

Cost of the feedstock

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16
Q

Stage 3 of design process

A

Sustainability of feedstock

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17
Q

Stage 4 of design process

A

Opportunity’s for recycling

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18
Q

Stage 5 of design process

A

Energy requirements

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19
Q

Stage 6 of design process

A

Marketability of by-products

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20
Q

Stage 7 of design process

A

Product yield( or atom economy)

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21
Q

Full design process

A 
Availablilty of feedstock
Cost of the feedstock
Sustainability of feedstock 
Opportunity’s for recycling 
Energy requirements 
Marketability of by-products
Product yield
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22
Q

Batch manufacturing

A

Advantages- suites for smaller scale production up to 100 tonnes per annum
- good for multistep reactions

Disadvantages- possibilities of contamination from one batch to the next
-filling and emptying takes time during which no Product is made = no money

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23
Q

Continuous manufacturing

A

Advantages-suites to large scale production up to >1000 tonnes per annum

  • suitable for fast single step processes
  • more easily controlled via computers

Disadvantages-much higher capital cost before production can begin

  • not versatile, can only make 1 product
  • not cost effective when run below full capacity
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24
Q

Capital costs

A
  • Research and development
  • plant construction
  • Buildings
  • infrastructures
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25
Q

Fixed costs

A

Depreciation of plants
Labour
Land purchase or rental
Sales experts

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26
Q

Variable costs

A

Raw material
Energy bills
Overheads
Efficient waste treatment

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27
Q

Factors influencing the process chosen

A

Availability And sustainably of feedstocks
Cost of feedstocks
Opportunity’s for recycling

28
Q

How does the availability and sustainability of feedstocks influence the process chosen

A

Salt water is widely available and supplies are unlimited

29
Q

How does the cost of feedstocks influence the process chosen

A

Salt water would have to be pumped to the plant

Water may have to be filtered

30
Q

How does opportunities for recycling influence the process chosen

A

I reacted sodium chloride solution would have to be separated from the sodium hydroxide and fed back to the plant

31
Q

What is green chemistry

A

Green chemistry is the sustainable design of chemical products and chemical processes. It minimises the use of chemical substances that are hazardous to human health of the environment

32
Q

Green chemistry principles

A

Better to prevent waste than to deal with it

Chemical processes should aim to incorporate all reactants in the final product

Chemical processes should aim to use and generate substances with minimal toxicity to human health and the environment

Modern chemists design reactions with the highest possible atom economy in order to minimise environmental impact.
Chemists achieve this by reducing raw materials and energy consumption

33
Q

What is the goal of atom economy

A

In an ideal reaction all reactant atoms end up within the useful product molecule
No waste is produced

34
Q

Inefficient, wasteful reactions have

A

Low atom economy

35
Q

Efficient processes have

A

High atom economy and are important for sustainable development as they create less waste

36
Q

A reaction may have

A

A high percentage yield but a low atom economy or vice versa

37
Q

What is a limiting reactant

A

A limiting reactant is the substance that is fully used up and thereby limits the possible extent of the reaction. Other reactants are said to be in excess

38
Q

Chemical reactions that take place in both directions are called

A

Reversible reactions

39
Q

The position of the equilibrium does not

A

Depend on the starting position

40
Q

What is a feedstock

A

A feedstock is a chemical from which other chemicals are manufactured. They are made from raw materials.

41
Q

Examples of raw materials

A 
Fossil fuels- coal, oil and natural gas
Metallic ores
Minerals- chlorine from sodium chloride 
Water and air
Organic materials
42
Q

Examples of products made from the batch process

A

Pharmaceuticals(medicines), dyes etc

43
Q

Examples of products made from continuous process

A

Sulphuric acid, ammonia, iron, ethene

44
Q

What are operating conditions

A

The conditions under which a chemical process operates to maximise economic efficiency

45
Q

What are capital costs

A

Capital costs is when you are building the plant

46
Q

What are fixed costs

A

These are costs that are the same wether 1 or 100tons of product are made

47
Q

What is excess

A

Reactants are needed for a chemical reaction to take place. When one of the reactants is used up the reaction will stop. Any reactant which is left I reacted is said to be in excess

48
Q

Equilibria(reversible reactions)

A

In a reversible reaction, if the conditions are not altered a balance point will be reached. At this point the reaction is said to be in equilibrium. At equilibrium the reactants change into products at exactly the same rate at which the products change back Into reactants.

49
Q

At equilibrium the concentrations of the reactants and products

A

Remain constant but not necessarily equal

50
Q

Changing concentration equilibrium

A

Increasing the concentration of reactants, or decreasing the concentration of the products shifts the position of the equilibrium to the right

Decreasing the concentration of reactants, or increasing the concentration of the products shifts the equilibrium to the left

51
Q

Changing temperatures equilibrium

A

Increasing temperature favours the endothermic reaction

Decreasing the temperature favours the exothermic reaction

52
Q

Catalyst equilibrium

A

A catalyst does not alter the position of equilibrium but does speed up the rate at which equilibrium is attained

53
Q

Definition of enthalpy of combustion

A

The enthalpy of combustion is the energy released to the surroundings when one mole of a substance burns completely in oxygen

54
Q

What can Hess’s law be used for

A

Hess’s law can be used to calculate enthalpy changes which are difficult or impossible to determine by experiment

55
Q

Enthalpy of formation definition

A

The enthalpy of formation is the quantity of heat energy taken in or given out when 1 mole of a substance is formed from its elements in its natural state

56
Q

What is a redox reaction

A

A redox reaction involves two half reactions- oxidation and reduction
These half reactions can be written as ion-electron equations

57
Q

What is oxidation

A

Oxidation is loss of electrons
OIL
The ion-electron equation for oxidation must be written in reverse

58
Q

What is reduction

A

Reduction is gain of electrons

RIG

59
Q

Oxidation and reduction are two half’s of

A

The same chemical reaction. The combined reaction is called a redox reaction

60
Q

What is an oxidising agent

A

In a redox reaction the thing that is reduced is the oxidising agent- the thing that allows oxidation to occur

61
Q

What is a reducing agent

A

In a redox reaction the thing that is oxidised is the reducing agent- the thing that allows reduction to occur

62
Q

What is chromatography

A

Chromatography is a method of separating and analysing a mixture of soluble chemical substances

63
Q

Uses of chromatography

A

Chromatography can be used to follow the course of a chemical reaction or to establish the products of a chemical reaction.

It can also be used to identify additives in food, analyse fibres found in crime scenes and fingerprints

64
Q

What are the two stages in paper chromatography

A

Mobile and stationary phase

The solvent is the mobile phase and wet paper is the stationary phase

65
Q

What is the retention factor

A

The retention factor can be used to compare the different components found in a sample.

If two substances have the same RF value it is likely that they are the same compound.

Higher Chemistry (2 decks)

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