C7

Front 1

Examples of bulk chemicals

Back 1

Ammonia, Sulfuric acid, Sodium hydroxide

Front 2

Examples of fine chemicals

Back 2

Drugs, food additives, fragrances

Front 3

How does the government protect people and the environment from chemical hazards

Back 3

Strict regulation of chemical processes and the transport and storage of chemicals

Front 4

What are the steps to producing a useful chemical?

Back 4

1) Preperation of feedstocks
2) Synthesis
3) Seperation of products
4) Handling of byproducts and wastes
5) Monitoring of purity

Front 5

The sustainability of chemical processes depends on...

Back 5

Use of renewable feedstocks, atom economy, by-products and wastes, energy inputs/outputs, environmental impact, health and safety risks...

Front 6

What is meant by the term 'activation energy'?

Back 6

The energy needed to break bonds to start a reaction

Front 7

What are catalysts?

Back 7

Catalysts are substances that reduce the activation energy of a reaction by providing an alternative route. They are not used up in the reaction so can be re-used.

Front 8

What are the optimum conditions for enzyme catalysts?

Back 8

Constant PH, temperature 30-40 degrees C

Front 9

How would you find the theoretical yield of calcium oxide produced from 50kg of calcium carbonate?

(CaCO3 -> CaO + CO2)

Back 9

use formula: Amount(A) /RFM (A) x RFM (B)

50kg/100 x 56= 28kg

Front 10

Name the first 4 alkanes and their chemical formulas.

Back 10

Methane (CH4), Ethane (C2H6), Propane (C3H8), Butane (C4H10)

Front 11

Alkane + Oxygen -> ?

Back 11

Carbon dioxide + Water

Front 12

Why don't alkanes react with aqueous reagents?

Back 12

They are saturated compounds- they contain only single bonds which are hard to break

Front 13

What is an unsaturated compound?

Back 13

A compound which contains atleast one couble C=C bond.

Front 14

Give two uses of Methanol and Ethanol.

Back 14

Methanol can be used as a chemical feedstock or to manufacture cosmetics. Ethanol can be used as a solvent or a fuel.

Front 15

What are the first 3 alcohols? Give their formulas.

Back 15

Methanol (CH3OH), Ethanol (C2H5OH), Propanol (C3H7OH)

Front 16

Give 2 properties of alkanes and explain them.

Back 16

Less dense than water (due to hydrocarbon chain)
Higher boiling point than alkanes (OH behaves like water)

Front 17

Alcohol + Oxygen -> ?

Back 17

Carbon dioxide + Water

Front 18

Ethanol + Sodium -> ?

Back 18

Sodium Ethoxide + Hydrogen

Front 19

What does a sodium reaction with an Alcohol/Water/Alkane look like?

Back 19

Alcohol= Sinks, doesn't melt, steady release of hydrogen
Water= Rushes around on the surface, melts, rapid release of hydrogen
Alkane= No reaction

Front 20

Give 3 ways of producing ethanol

Back 20

Synthesis, Fermentation, Bacteria

Front 21

Give the reaction for producing ethanol by synthesis and the conditions required for this

Back 21

Ethene + Steam -> Ethanol

Sulfuric acid catalyst, high temperature, high pressure

Front 22

Give the reaction for producing ethanol by fermentation and the conditions required for this

Back 22

Water + Sugars + Yeast -> Ethanol + Carbon dioxide

Constant PH, Temperature 30-40 degrees C

Front 23

Why is there a limit to the concentration of ethanol produced by fermentation? How can the concentration be increased?

Back 23

The concentration is limited by the sugar in the mixture and the enzymes in the yeast. It can be purified through distillation to produce spirits such as whisky and brandy.

Front 24

Give the reaction for producing ethanol through biotechnology and the conditions required for this

Back 24

Water + Sugar from waste biomass + GM E.coli -> Ethanol + Carbon dioxide

Constant PH, Temperature 25-37 degrees C

Front 25

List some disadvantages of each of the fermentation techniques

Back 25

Synthesis: Use of crude oil (unsustainable), High temperature/pressure required.
Fermentation: Use of land to grow feedstock sugars, Carbon dioxide produced as byproduct
Biotechnology: Carbon dioxide produced

Front 26

Give the formula for Methanoic and Ethanoic acid.

Back 26

Methanoic (HCOOH), Ethanoic (CH3COOH)

Front 27

Give a distinctive property of Carboxylic acids and where this can be found.

Back 27

Strong unpleasant smells eg: Rancid butter/Sweaty socks

Front 28

Ethanoic Acid + Sodium -> ?
Propanoic Acid + Sodium hydroxide -> ?
Methanoic Acid + Sodium carbonate -> ?

Back 28

Sodium ethanoate + Hydrogen
Sodium propanoate + Water
Sodium methanoate + Water + Carbon dioxide

Front 29

Give the formula for the production of esters

Back 29

Alcohol + Carboxylic acid -> Ester + Water

Front 30

Give a property and some uses for esters

Back 30

Esters have distinctive smells, eg: those in fruits. They are used as food flavourings, solvents, plasticizers, and in perfumes

Front 31

Give the steps for the production of an ester

Back 31

1) Heating under reflux
2) Distillation
3) Purification with sodium carbonate (tap funnel)
4) Drying with anhydrous calcium chloride (filtration

Front 32

Give the reaction for the production of fats

Back 32

Glycerol + Fatty acids -> Fats + Water

Front 33

What do plants and animals use fats for and what types do they produce?

Back 33

As a store of energy

Plants/vegetables: mostly unsaturated
Animals: mostly saturated

Front 34

What is meant by the terms endothermic/exothermic?

Back 34

Endothermic = takes in energy from surroundings
Exothermic= releases energy to surroundings

Front 35

What is a dynamic equilibrium?

Back 35

When the rates of the forwards and backwards reactions are the same so there is no overall change

Front 36

Give the reaction for the Haber process and the conditions required

Back 36

Nitrogen + Hydrogen <-> Ammonia

Iron catalyst, High temperature (450 degrees C), High pressure (200 atmospheres)

Front 37

What are the advantages/disadvantages of using very high pressures in the Haber process?

Back 37

High pressures push the equilibrium towards the products so increase the percentage yield. However this needs to be balanced by the fact that high pressures are expensive to create.

Front 38

What are the advantages/disadvantages of using very high temperatures in the Haber process?

Back 38

High temperatures push the equilibrium towards the reactants so decrease the percentage yield. However, high temperatures increase the rate of reaction.

Front 39

How is the percentage yield of the Haber process increased?

Back 39

Hydrogen and Nitrogen are recycled and reused.

Front 40

How else can nitrogen be fixated (other than the Haber Process) ?

Back 40

Nitrogen-fixing bacteria naturally convert nitrogen into ammonia at room temperature and pressure using enzymes as catalysts. Scientists are eager to replicate this.

Front 41

What does qualitative/quantitative analysis tell you?

Back 41

Qualitativ tells you which compounds are present
Quantitive tells you how much is present

Front 42

What are standard procedures?

Back 42

Guidelines for the collection, storage and preparation of samples for analysis to prevent contamination/inaccurate results.

Front 43

What is chromatography and what is it used for?

Back 43

Chromatography is where a sample is placed at an equilibrium between a stationary phase and a mobile phase. It is used to identify different materials, based on the distribution between the two phases.

Front 44

What are the mobile/stationary phases in paper chromatography?

Back 44

Mobile phase= water
Stationary phase= paper

Front 45

What are the mobile/stationary phases and in TLC and what are its advantages over paper chromatography?

Back 45

Mobile phase= water
Stationary phase= silica gel on glass plate

TLC is faster and more even than paper chromatography, and can be used for a wider range of substances

Front 46

How do you calculate the Rf value of a substance?

Back 46

Distance traveled by solute/distance traveled by solvent

Front 47

What are the mobile/stationary phases in gas chromatography?

Back 47

Mobile phase= carrier gas
Stationary phase= microscopic layer of liquid in glass/metal column

Front 48

Give some advantages of gas chromatography over TLC or paper chromatography

Back 48

- Greater separating power
- Can separate complex mixtures
- Can produce quantitative data from very small samples

Front 49

What does the size of peak and retention time tell you on a gas chromatogram?

Back 49

Retention time tells you what substance it is
Size of peak tells you how much is present

Front 50

What are the stages of quantitative analysis?

Back 50

1) Take a representative sample
2) Accurately measure out and dissolve the sample
3) Measure a property of the solution and calculate a value
4) Estimate the degree of uncertainty

Front 51

How do you produce a standard solution?

Back 51

1) Weigh out the solid sample in a beaker
2) Transfer the solid to a volumetric flask- wash the funnel with distilled water so no solid is lost
3) Add distilled water until the flask is 3/4 full and shake
4) On a level surface, carefully fill with water until the water line is at the bottom of the meniscus
5) Invert the flask to ensure an even concentration

Front 52

How would you calculate the concentration of an acid (A) after a titration with an alkali (B)

Back 52

Mass (B) x RFM(B)
----------------------------
Volume(A) x RFM(A)

Front 53

What is the formula for calculating mass with a known volume and concentration?

Back 53

Mass= Volume x Concentration

Front 54

How do you calculate percentage uncertainty?

Back 54

range of results
---------------------- x 100
mean of results

Front 55

What is a locating agent

Back 55

A locating agent eg: UV light/coloured dyes allows you to identify the distribution of the substance

Front 56

What are the steps to carry out a titration?

Back 56

1) Fill a burette with alkali of known concentration/volume
2) Measure set volume of acid into a flask and add indicator
3) Add the alkali drop by drop, swirling the flask
4) Record the volume of alkali required to neutralise the acid, and repeat