Electrode potentials snd electrochemical cells 3.1.11 Flashcards

1
Q

what is a half cell

A

One half of an electrochemical cell . they can be constructed of a metal dipped in its ions , or a platinum electrode with 2 aqueous ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is an inert but electrically conductive electrode commonly used

A

platinum

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

how is an electrochemical cell created

A

by joining 2 different half cells together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what are electro cells made up of

A

2 half cells joined by a wire voltmeter and a salt bridge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what does a voltmeter do

A

•Measures voltage between two half cells . Known as the emf
• electrons flow from a more reactive metal to a less reactive one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is a salt bridge made out of

A

filter paper with potassium nitrate solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what does a salt bridge do

A

The ions in the ionic substance in the salt bridge move through the salt bridge .
To complete the circuit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what does the electrode potential value measure

A

tells us how easily the half cell gives up electrons ( oxidised )

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

how can you tell which half cell is being reduced or oxidised

A

Look at the their electrode potential value from the data book

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what if the electrode potential value is negative

A

it undergoes oxidation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what if the electrode potential value is positive

A

undergoes reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what is the standard hydrogen electrode

A

Is used to as a reference to measure standard electrode potentials

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what’s the electrode potential value for the standard hydrogen electrode

A

0.00V

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what are the general conditions and set ip for the standard hydrogen electrode

A
  • H2(g) in at 298K and 100KPa
  • 1 moldm-^3 of Cu2+ ions ( solution)
  • 1 moldm-3 of H+ ions (solution)
  • Platinum electrode
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is the electrochemical series

A

A list of electrode potentials in numerical order

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What order can the electrochemical series be in

A

either ascending or descending order

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what are oxidising agents

A

increasing tendency to gain electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

which half cell reactions would be stronger oxidising agents

A

The ones with a more positive electrode potential

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

if the electrochemical series was in descending order which parts of the half cell reactions would be an oxidising agent or a reducing agent

A

-agents on the left hand side of the equation are more easily reduce so they are more powerful oxidising agents
- agents in the right hand side of the equation are more easily oxidised so they are more powerful reducing agents

20
Q

what is a reducing agent

A

They have an increasing tendency to lose electrons

21
Q

what is the equation to work out the cell potential

A

E cell = E reduced ( most positive) - E oxidised ( most negative )

22
Q

what are cell notations

A

Used to simplify how we draw the set up of cell . They are the standard way of representing cells in chemistry

23
Q

what’s the general way of writing cell notation

A

Reduced form | oxidised form | | oxidised form | reduced form
( the most negative half cell potential goes to the left of the double line )

24
Q

what does the solid line in a cell notation represent

A

Show a physical change in state e.g solid to gas

25
Q

what do double solid lines show in a cell notation

A

a salt bridge

26
Q

what if there are 2 aqueous ions in a half cell how would you represent that in a cell notation

A

Separate ions with a comma

27
Q

what can standard electrode potentials be used for

A

to predict if a stated reaction is likely to proceed under standard conditions

28
Q

what do we do with an oxidation equation

A

have to reverse it

29
Q

what are the steps to predict feasibility in reactions

A

1) identify which is being oxidised
2) take the oxidised equation and reverse it. Write two equations next to each other
3) combine the 2 equations to obtain a feasible reaction
4) compare this equation to the reaction stated in the question
5) confirm this by calculated the E cell . All feasible reactions will have a positive E cell value

30
Q

how can you tell if a reaction is feasible

A

work out E cell.
All feasible reactions will have a positive E cell value

31
Q

what are batteries

A

electrochemical cells that come in 2 main forms . rechargeable and non- rechargeable

32
Q

what are some features of non rechargeable batteries

A

• tend to be cheaper than rechargeable batteries.
however rechargeable batteries are reversible and can last longer so cheaper in the long term

33
Q

what are lithium ion batteries

A

an example of a rechargeable battery.

34
Q

what are lithium ion batteries commonly used in

A

wireless power tools
tablets
mobile phones
electric cars

35
Q

what are the components of a mobile phone that use a lithium ion cell

A

Electrode A - lithium cobalt oxide (LiCoO2)
Electrode B - graphite (C)
Electrolyte - Lithium salt dissolved in an organic solvent

36
Q

how do rechargeable batteries work

A

Plugging them in to supply a current
This current forces electrons to flow in the opposite way
all we do is reverse the overall discharge equation to show a battery recharging it

37
Q

what is a fuel cell

A

electricity generated by a continuous external supply of chemicals rather than a “ready store” like in batteries

38
Q

what’s an example of a fuel cell

A

an alkaline hydrogen - oxygen fuel cell

39
Q

what are the stages that happens in an alkaline hydrogen-oxygen fuel cell

A

1) Hydrogen feed
Hydrogen is fed here. It reacts with OH- ions in solution. The reaction :
2H2(g) + 4OH-(aq) => 4H2O(l) + 4e-
2) Flow of electrons
Electrons produced in reaction 1 travel through a platinum electrode. Platinum is a good conductor of electricity but inert.
3) Component
The flow of electrons is used to power something
4) Oxygen Feed
Oxygen is fed in here. It reacts with water and the 4 electrons made from step 1 to make OH- ions.
The reaction : O2(g) + 2H2O (l) + 4e- => 4OH- (aq)
5) Negative electrode (cathode)
Electrons flow to the negative electrode which is made from platinum
6) Electrolyte
The electrolyte is made from KOH solution . It carries the OH- ions from the cathode to the anode
7) Positive electrode (anode)
Electrons flow from the positive electrode which is made from platinum
8) Water emitted
The product of the reaction in step 1 is released into the surroundings
9) Movement of OH- ions
OH- ions produced from reaction 4 are carried towards the anode via the electrolyte

40
Q

what are Ion exchange membranes in an alkaline hydrogen-oxygen fuel cell

A

These lines on the platinum electrodes and these allow OH- pins to pass through but NOT hydrogen and oxygen gas

41
Q

what are the reactions taken place in an alkaline hydrogen - oxygen fuel cell

A

Half equations :
2H2 (g) + 4OH- (aq) => 4H2O(l) + 4e-
O2 (g) + 2H2O(l) + 4e- => 4OH-(aq)

Overall equation :
2H2(g) + O2(g) => 2H2O

42
Q

What are advantages of fuel cells

A

• more efficient
• more energy is converted into kinetic energy
• fuel cells don’t need to be recharged ~ you just need a ready supply of oxygen and hydrogen
• the only waste product is water and no co2 emitted directly from the cell unlike a combustion engine

43
Q

what are some disadvantages of fuel cells

A

• hydrogen is highly flammable and must be stored and transported correctly
• It is expensive to transport and store hydrogen. Storage of hydrogen is in pressurised containers
• energy is required to make the hydrogen and oxygen in the first place.
Fossil fuels are generally used to pass water through an electrolysis process. the use of fossil fuels contributes to CO2 emissions

44
Q

EQ : An Emf Value for a commercial lithium-iodine cell is 2.80V
Suggest why this value is different from the value calculated in part (b) (1)

A

Non - standard conditions

45
Q

Equation for the reaction that occurs at the positive lithium cobalt oxide electrode

A

Li^+ + CoO2 + e^- => LiCoO2