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Chemistry > S5 - Unit 3 > Flashcards

S5 - Unit 3 Flashcards

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1
Q

What do industrial processes aim to do?

A

Maximise profit, minimise environmental impact

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2
Q

How do you make a standard solution?

A
  • Weigh the solid into a small, clean beaker
  • Dissolve in a small volume of water
  • Transfer to a volumetric flask
  • Make it up to the graduation mark with water
  • Insert a stopper and invert several times to mix
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3
Q

What is a limiting reactant?

A

The reactant used up in a reaction which determines the mass of product formed

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4
Q

What is percentage yield?

A

The amount of product you actually make as a percentage of the amount you should theoretically make

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5
Q

What is atom economy?

A

A measure of the percentage of reactants that become useful products

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6
Q

Why must reaction rates be controlled in industrial processes?

A

Because if reaction rates are too high there will be the risk of explosion and if they’re too low the process will not be economical

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7
Q

What factors affect the rate of reaction?

A
  • Concentration
  • Particle size
  • Temperature
  • Pressure
  • Collision geometry
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8
Q

What does it mean if a reaction is at equilibrium?

A

The rate of the forward reaction is equal to the reverse reaction

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9
Q

What happens when equilibrium is reached?

A

The concentrations of products and reactants remain constant

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10
Q

What factors affect the position of equilibrium?

A
  • Concentration
  • Particle size
  • Temperature
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11
Q

What do catalysts do to the equilibrium?

A

Nothing, they only help reach equilibrium faster

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12
Q

What will happen when there is an increase in pressure when a reaction is in a state of equilibrium?

A

Will favour the side with the least gas moles

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13
Q

What will happen when there is an increase in temperature when a reaction is in a state of equilibrium?

A

Will favour the endothermic side

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14
Q

What will happen when there is an increase in a certain element when a reaction is in a state of equilibrium?

A

Will favour the side with the smaller volume of that element

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15
Q

What will happen when there is a decrease in pressure when a reaction is in a state of equilibrium?

A

Will favour the side with more gas moles

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16
Q

What will happen when there is a decrease in temperature when a reaction is in a state of equilibrium?

A

Will favour the exothermic side

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17
Q

What will happen when there is a decrease in a certain element when a reaction is in a state of equilibrium?

A

Will favour the side with the larger volume of that element

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18
Q

What will happen when an alkali is added to an equilibrium reaction?

A

The H ions will be removed

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19
Q

What will happen when an acid is added to an equilibrium reaction?

A

The H ions will increase

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20
Q

What must happen before products can be formed?

A

Reactant molecules must collide in the correct way

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21
Q

What do the collisions of reactant molecules provide?

A

The energy needed to break the bonds between them and the energy needed to form the bonds on the new products

22
Q

What factors must be present at the same time for a reaction to be successful?

A
  • Sufficient energy
  • Correct geometry
23
Q

What is activation energy?

A

The minimum kinetic energy required for a reaction to occur

24
Q

What type of reaction has taken place in the diagram?

A

Exothermic

25
Q

What type of reaction has taken place in the diagram?

A

Endothermic

26
Q

What are the blanked out words?

A
27
Q

What are the blanked out words?

A
28
Q

What is the enthalpy of combustion?

A

The heat energy given out when 1 mole of fuel burns completely in oxygen

29
Q

What is the enthalpy of solution?

A

The energy change when 1 mole of a substance dissolves completely in water

30
Q

What is enthalpy of neutralisation?

A

The heat energy given out when 1 mole of water is formed in a neutralisation reaction

31
Q

What does Hess’ law state?

A

The enthalpy change for a reaction is independent of the route taken

32
Q

What is the enthalpy of formation?

A

The energy needed to make 1 mole of a compound from its elements in their standard state

33
Q

What type of reaction is the breaking of bonds?

A

Endothermic

34
Q

What type of reaction is the making of bonds?

A

Exothermic

35
Q

What is the symbol that represents an exothermic reaction?

A

-ΔH

36
Q

What is the symbol that represents an endothermic reaction?

A

+ΔH

37
Q

What is chromatography?

A

An important analytic technique which allows chemists to separate substances and identify unknown substances

38
Q

How does chromatography work?

A

Substances are separated as they travel in a mobile phase which passes through a stationary phase

39
Q

What are the two phases in paper chromatography?

A

Stationary; a sheet of chromatography paper

Mobile; water

40
Q

What is an advantage of thin layer chromatography?

A

The mobile phase moves more quickly through the stationary phase

41
Q

What is gas chromatography used for?

A

To separate complex mixtures

42
Q

What factor effect retention time?

A
  • polarity
  • volatility
  • mass of a substance
43
Q

How do you calculate the enthalpy change for a forward reaction?

A

Products - reactants

44
Q

How do you calculate the enthalpy change for a reverse reaction?

A

Reactants - products

45
Q

What is an activated complex?

A

An intermediate state where particles can either form products or go back to particles of the reactants

46
Q

What do catalysts do to the activation energy?

A

Lower the activation energy

47
Q

What are the principles of chemical industry design?

A

Availability, cost and sustainability of feedstocks

48
Q

What is considered to be a raw material in the chemical industry?

A
  • fossil fuels
  • water
  • air
  • metal ores
  • minerals
49
Q

What are feedstocks in the chemical industry?

A

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

50
Q

What is considered in the chemical industry?

A
  • what the cost is
  • if the feedstocks are sustainable
  • if any by-products can be recycled

Chemistry (7 decks)

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