ELECTRODE POTENTIAL Flashcards

1
Q

Half cell

A

a half cell is one half of an electrochemical cell. they can be constructed of a metal dipped in its own ion or a platinum electrode in 2+ aqueous ions.

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2
Q

why do we use platinum electrode

A

because it is inert and electrically conductive metal.

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3
Q

electrochemical cells

A

electrochemical cells are made up of two half cells joined together by a wire, a voltmeter and a salt bridge. there are always two reaction occuring oxidation and reduction therefore it is a redox reaction.

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4
Q

what is a salt bridge

A

strip of a filter paper soaked in kno3 solution.

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5
Q

how do electrons flow between half cells

A

always from a high recating metal to the lower one.
example zinc gets oxidised and gets thinner whereas copper gets reduced and becomes thicker.

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6
Q

electrode potential or delta e

A

each half cell has its own electrode potential. it tells us how easily the half cell gives up electrons ( becomes oxidised)

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7
Q

how do we write up the equations

A

always in reduced form. never in oxidised form.n

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8
Q

acronym we use

A

NO PROBLEM
the most negative value is oxidised meaning that equation needs to be flipped
and the most positive value is the one getting reduced.

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9
Q

SHE stands for?

A

STANDARD HYDROGEN ELECTRODE

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10
Q

SHE ( STANDARD HYDROGEN ELECTRODE)

A

SHE is a reference for measuring standard electrode potential.

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11
Q

value of SHE

A

0.00VOLTS

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12
Q

What affects the value of an electrode potential

A

temperarure, pressure and concentration

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13
Q

standard conditions?

A

temperature – 298K
Pressure – 100Kpa
concentration– 1mol per dm -3.

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14
Q

note

A

when we say concentration we actually mean, 1 mol dm-3 of H+ ion not actually acid. if we use h2so4, then we use 0.5 mol dm-3 since its a diprotic acid.

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15
Q

electro chemical series

A

electro chemical series is a list of half cell reactions and their standard electrode potentials.

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16
Q

oxidisation and oxiding agent

A

oxifdation is losing electron and oxidising agent is gaining electron

17
Q

reduction ans reducing agent

A

reduction is gaining electron and reducing agent is losing electron

18
Q

note for electro chemical series

A

in an electro chemical series, we always find the oxidising agent in the left hand side and the reducing agent always on the right hand side.

19
Q

standard cell potential

A

e reduced - e oxidised.

20
Q

cell notation

A

standard way of representing cells in chemistry.

21
Q

cell notation format

A

reduced form l oxidised form ll oxidised form l reduced form

where ll represents a salt bridge
and l represents a physical state change.

22
Q

what do we do if we have two aqueous ions

A

we use a comma

23
Q

batteries

A

batteries are electro chemical cells that exists in two forms : rechargeable and non rechargeable.

24
Q

example of rechargeable battery

A

lithium ion batteries used in phone etc.

25
Q

note

A

mobile phone uses a lithium ion cell havin the folowing components
electrode A - LITHIUM COBALT OXIDE
electrode B - GRAPHITE
ELECTRODE - lithium salt dissolved in organic solvent.

26
Q

steps to find a reaction feasibility

A
  1. from the electro chemical series find out the oxidised reaction, remember NO PROBLEM (most negative is oxidised)
  2. after finding the oxidised equation, always flip it,(it will be in reduced form in the equation)
  3. after flipping the oxidised equation, make sure number of electrons are equal in both reactions and cancel out the electrons.
  4. write out the remaining bits to see if they match.
  5. you can also find electrode potential with the formula
    reduced - oxidised ( acronym redox)
  6. if the value is positive, it means that the reaction is feasible.