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Higher Chemistry > Chemistry In Society > Flashcards

Chemistry In Society Flashcards

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1
Q

How to increase rate of reaction

A

Decrease particle size, increase temperature, increase concentration of acid

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2
Q

How to decrease rate of reaction

A

Increase particle size, decrease temperature, decrease concentration of acid

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3
Q

What are the pros of increasing/decreasing rate of reaction

A

Increase- it happens quicker so more profit

Decrease- increases safety as it reduces the risk of thermal explosion

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4
Q

What happens in the Ostwald Process

4NH(3) g+ 5O(2) g ➡️ 4NO g + 6H(2)O g

A

Occurs at 900C
~96% conversion of ammonia
Highly Exothermic
Temperature rise can be dangerous as it can damage the platinum-rhodium catalyst

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5
Q

What is collision theory

A

It’s how the reactants are brought together and collide with each other

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6
Q

What is the link between temperature and kinetic energy

A

The temperature is the average kinetic energy so an increase in temp is an increase Ке

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7
Q

What are the stages of production for a new product

A
  • Research and Development- includes selection of the most suitable rumours for production
  • Lab Process - small scale- review and modify the selected route
  • Pilot Plant - medium scale - reviews quality, health hazards and engineering costs
  • Production Plan - Plant Design, construction, commissioning and start up
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8
Q

What factors must be assessed when creating a new product

A 
Availability, sustainability and cost of feedstock
Opportunities for recycling
Energy requirements 
Marketability of by-products
Product yield / atom economy
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9
Q

How can you reduce the cost of feedstock

A

If the source can be sourced locally it is useful as this can reduce cost and increase profits

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10
Q

How can profits be maximised through recycling

A

Unreacted starting materials can be fed back into the reaction to reduce cost, making it more economical

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11
Q

How can profit be lost when sourcing and buying feedstock

A
  • Can cost a lot to transport the feedstock from further away
  • the rarity and availability of a material can increase the cost as more rare materials cost more
  • The price of things like oil and a gas fluctuate
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12
Q

How can profit be lost in the recycling process

A

It can sometimes be very expensive to see rate unreacted materials

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13
Q

Where can extra profit be made with energy requirements

A

Exothermic reactions heat up other reaction so the can be used instead to save money on energy costs

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14
Q

What is the industrial process designed to do

A

Maximise profit and minimise the effect on the environment

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15
Q

Why are the two ways products are produced in the chemical industry

A

Batch and continuous

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16
Q

The pros of batch production

A

Can produce up to 100 tonnes per annum
More versatile
Good for multi step reactions

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17
Q

The cons of batch production

A

Contamination is more likely
At times no product is produced
Safety is more of an issue

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18
Q

The pros of continuous production

A

Can produce up to 1000 tonnes per annum
Good for fast single step process
Easy to automate

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19
Q

Cons of continuous production

A

Capital cost is high
Less flexible
Needs to run at full capacity to make profit

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20
Q

How does fractional distillation work

A

Volitle ( small particles) are at the top
Viscous (large particles) are at the top
Bitumen is left over at bottom
Gasses are Volitle
Things are split based on their boiling point

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21
Q

What is green chemistry

A

The sustainable design of chemical product and processes

Minimises the use and generation of martial chemical substance

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22
Q

What are the principle of design for cost

A
  • capitol cost - fixed/variable cost
  • research and development- depreciation if plant/raw materials
  • plant construction - Labour/Energy bills
  • buildings-land purchase or rental/overheads
  • infrastructure-sales expenses/effluent waste treatment
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23
Q

Is a high or low Percentage yield better in a business

A

high percentage yield as it makes more profit

24
Q

What is the statement that should be made for when 10g of calcium carbonate reacts in excess with 100cm3 of 1mol l-1 of hydrochloric acid

A

The molar ratio between HCl:CaCO3 is 2:1. In this reaction we have 0.1 miles of HCl and 0.1 miles of CaCO3. CaCO3 is in excess because if we have 0.1 miles of HCl we only need 0.05 miles of CaCO3

25
Q

What is a reversible reaction

A

A reaction that take place in both directions

Reactants↔️Products

26
Q

What is equilibrium

A

It is when the rate of forward reaction is equal to the rate of the reverse reaction

27
Q

Does the starting point of a reaction affect it’s equilibrium

A

No

28
Q

What happens if you alter one of the factors in a reaction (pressure, temperature , concentration)

A

The equilibrium will shift to attempt to undo any changes imposed on it

29
Q

What happens to the concentration of product and reactants at equilibrium

A

They stay the same

But the concentration of reactants won’t always equal the concentration of products

30
Q

How does equilibrium shift when an exothermic reaction is heated up

A

It shifts to the left

31
Q

How does equilibrium shift when an exothermic reaction is cooled down

A

It moves to the right

32
Q

How does equilibrium shift when an endothermic reaction is heated up

A

It moves to the right

33
Q

How does equilibrium shift when an endothermic reaction is cooled down

A

It moves to the left

34
Q

How does equilibrium shift when the pressure on a gas is increased

A

It shifts towards the side with less moles of gas

35
Q

How does equilibrium shift when the pressure on a gas is decreased

A

It shifts to the side with more moles of gas

36
Q

How does equilibrium shift in a reaction when either reactants are added or products are removed

A

It shifts to the right

37
Q

How does equilibrium shit in a reaction when either reactants are removed or products are added

A

It shifts to the left

38
Q

What is Hess’s law

A

It states that the enthalpy change of a chemical reaction does not depend on the route taken during the reaction

39
Q

How can you verify Hess’s Law

A 
KOH(s) ——🔼H1———>KCl(aq)
      ↘️.                                 ↗️
🔼H2↘️ +H2O(l).          ↗️ HCl(aq)🔼H3
              ↘️.                ↗️
                     KOH(aq)
       🔼H1=🔼H2 +🔼H3
40
Q

What is volumetric analysis

A

It involves using a solution of a known and accurate concentration in a quantitive reaction to determine the concentration of an unknown substance

41
Q

How close do accurate titres have to be to be concordant

A

0.2ml

42
Q

What is a standard solution

A

A solution with an accurate and known concentration

43
Q

What is a redox titration

A

Titrations that are based on redox equations

44
Q

Is an indicator needed when potassium permanganate is used

A

No as it turns colourless

45
Q

What is Chromatography

A

It is used to split different compounds by their solubility

46
Q

What is the retention factor(rf)

A

It’s how soluble a substance is in the solvent

a bigger number meaning that the dot travelled further/ is retained more

47
Q

What are the uses of chromatography

A

Forensics, immigration disputes, illegal trades
paternity
Looking for performance enhancing drugs/doping

48
Q

What is the reducing agent in redox equations

A

It is the one losing electrons so the chemicals that are oxidised

49
Q

What is the oxidising agent in redox equations

A

It is the chemicals that gain electrons so the chemicals that are reduced

50
Q

What does OILRIG mean

A 
Oxidation
Is
Loss
Reduction
Is
Gain
51
Q

What is displacement

A

It is when a metal is added into an equation and pushes out (displaces) a less reactive metal (in the electrochemical series) from the solution

52
Q

What are metals (on the LHS of the periodic table )called during redox

A

Reducing agents as they are oxidised (lose electrons)

53
Q

What are non metals called (on the RHS of the periodic table) in a redox equation

A

Oxidising agents as they are reduced (gain electrons)

54
Q

Which metals in the electrochemical series are oxidised and which are reduced

A

The metal higher in the electrochemical series is oxidised as it loses electrons and the one lower is reduced as it gains electrons

55
Q

What connects a half cell

A

A salt (ion) bridge

56
Q

How do you balance a redox equation

A

Make sure the number of atoms of each element being oxidised or reduced on each side of the half equation are balance
⬇️
If there are any oxygen atoms present, balance them by adding H2O to the other side of the half equation
⬇️
If there are any hydrogen atoms present balance them by adding H+ to the other sides
⬇️
Make sure the half reaction have the same overall charge on each side by adding electrons(e-)

Higher Chemistry (3 decks)

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