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Higher Chemistry > Unit 2- Chemistry In Society > Flashcards

Unit 2- Chemistry In Society Flashcards

1
Q

What is the laboratory process for producing a new chemical?

A

A small scale investigation to review and modify the selected route

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2
Q

What is the pilot plant stage in producing a new chemical?

A

Medium scale investigation of product quality

Health hazards and engineering costs are assessed

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3
Q

What are the 7 principles of design process?

A

Availability of feedstocks

Cost of feedstocks

Sustainability of feedstocks

Opportunities for recycling

Energy requirements

Marketability of by-products

Product yield(or atom economy)

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4
Q

What are feedstocks?

A

Simple chemicals or mixtures of chemicals derived from raw materials used in further manufacture

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5
Q

What is atom economy?

A

A measure of the proportion of the total mass of all starting materials converted into the desired products

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6
Q

What are raw materials?

A

Fossil fuels, water, air, metal ores and minerals.

These must be converted to feed stocks before being passed into a reactor

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7
Q

What are the 2 types of reaction sequences used in chemical industry?

A

Batch and continuous

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8
Q

Compare batch and continuous manufacturing

A

Batch- good for multi step reactions
More versatile

          Product contamination is more likely 
          Safety is more of an issue

Continuous- good for fast single step reactions
Easy to automate

                     Capital cost is high. 
                      Less flexible 
        Need to run at full capacity to make a profit
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9
Q

What is an example of a batch process?

A

Drug development

Whiskey production

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10
Q

What is an example of a continuous process?

A

Plastics

Blast furnace

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11
Q

Give an example of a capital cost.

A

Research and development
Plant construction
Buildings
Infrastructures

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12
Q

What are the uses for chromatography?

A

Dna tests

Doling tests

Blood identification testing

Ivory identification

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13
Q

Where are the strongest oxidation agents found in the periodic table?

A

Group 7

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14
Q

Give an example of variable costs

A

Raw materials
Energy bills
Overheads
Effluent waste treatments

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15
Q

What must be considered in the production of a chemical?

A

Operating conditions

Energy consumption

Environmental issues

Safety

Can the by-products be sold?

Cost of waste disposal

Yield and atom economy

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16
Q

What is the production plant stage in producing a new chemical?

A

Plant design, construction, commissioning and start up

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17
Q

What does percentage yield show?

A

The efficiency with which reactants are converted into the desired products

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18
Q

What is molar volume?

A

The volume occupied by one mole of gas

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19
Q

What is an equilibrium?

A

When the rate of the forward and reverse reaction in a reversible reaction are equal

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20
Q

What side will be favoured if the pressure is increased in a reaction at equilibrium?

A

The side with less moles of gas

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21
Q

What happens to the concentration of reactants once a reaction hits equilibrium?

A

Concentration remains constant

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22
Q

Are the concentration of reactants and products equal in an equilibrium reaction?

A

Rarely

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23
Q

What type of reaction is this?

————————————> -ve

A

Exothermic

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24
Q

What happens to a system at equilibrium that is subject to a change?

A

The system readjusts itself to counteract the change

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25
What side will a reaction at equilibrium favour if there is a rise in temp?
Endothermic to cool the reaction down
26
What side will a reaction at equilibrium favour if there is a drop in temp?
Exothermic to heat the reaction up
27
What is oxidation?
Loss of electrons
28
What side will a reaction at equilibrium favour if the concentration of REACTANTS is increased?
The forward reaction
29
What side will a reaction at equilibrium favour if the concentration of PRODUCTS is increased?
The reverse reaction
30
What is the one case in which changing the pressure of a reaction will not effect equilibrium?
If the number of moles of gas on each side of the equation are equal.
31
What side will be favoured if the pressure is decreased in a reaction at equilibrium?
The side with more moles of gas
32
What happens if a catalyst is added to a reaction at equilibrium?
The activation energy for both the foraged and reverse reaction is lowered and the rate of reaction is increased to the same extent. No effect on the position of equilibrium
33
What is Hess’s law?
Hess’s law states that the enthalpy change for a chemical reaction is independent for the route taken
34
What is enthalpy?
A measure of the chemical energy in a substance
35
What is an exothermic reaction?
A reaction or process that releases heat energy
36
What is an endothermic reaction?
A reaction or process that takes in heat energy
37
What is the retention factor?
How soluble your test substance is in the solvent The more soluble the bigger the number, and the further the dot will have travelled
38
What is the enthalpy of solution?
The energy change when one mole of substance is dissolved in water
39
Why is the enthalpy of neutralisation?
The energy change when acid is neutralised to form one mole of water
40
What relationship is used in to determine enthalpy changes scientifically?
E(h) =cm/\T
41
What errors can be found when measuring enthalpy with a spirit burner?
Draughts Heat absorption by the can Incomplete combustion (especially when trying to keep out draughts)
42
What are the 2 methods of measuring enthalpy experimentally?
Spirit burner Bomb calorimeter
43
What is enthalpy of combustion?
The enthalpy change when one mole of a substance burns completely in oxygen
44
What is the molar bond enthalpy?
The energy required to break one mole of bonds in a diatomic molecules in the gaseous state
45
What is reduction?
Gain of electrons
46
What is an oxidising agent?
A substance that accepts electrons, that is reduced, and assists oxidation
47
What is mean molar bond enthalpy?
The average energy required to break one mole of bonds for a bond that occurs in a number of compounds
48
What is a reducing agent?
A substance that donates electrons, that is oxidised, that will assist reduction.
49
Do elements with high or low electronegativities tend to act as oxidising agents?
High
50
Do elements with high or low electronegativities tend to act as reducing agents?
Low
51
Where are the strongest reducing agents found in the periodic table?
Group 1
52
Give an example of a fixed cost
Depreciation of plant Labour Land purchase and rental Sales expenses
53
What is the molar volume triangle
V _________ N | Mv
54
What are the advantages of the bomb calorimeter method of measuring enthalpy?
No draughts Less heat lost to the environment Controlled oxygen levels rather than air so complete combustion
55
What is an example of a reducing agent?
Carbon monoxide
56
What is an example of an oxidisation agent?
``` Hydrogen peroxide Or Dichromate ions Or Permanganate Ions ```
57
What is a common use for oxidising agents?
To kill fungi and bacteria | Or inactivate viruses
58
What is chromatography?
A technique used by scientists to split up different compounds that have different solubilities
59
What is the relationship between solubility and distance travelled in chromatography?
The more soluble the compound the further it will travel
60
What is the relationship for retention factor?
R=b/a
61
What are the 4 stages of manufacturing a new chemical?
Research and development Laboratory process Pilot plant Production plant
62
How do you make a standard solution?
Weigh out the solid Dissolve the solid in a small amount of solvent Fill to the solvent line (graduated mark)
63
What is the research and development stage in producing a new chemical?
Selection of the most suitable route for producing the new chemical
64
What are standard solutions?
Solutions of known concentrations made in volumetric glassware
65
What type of reaction is this? ————————————> +ve
Endothermic
66
What is volumetric analysis?
The use of a solution of accurately known concentration in a quantitative reaction to determine the concentration of another substance

Higher Chemistry (3 decks)

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