EMF Flashcards

1
Q

what is electrode potential a measure of?

A

oxidising ability

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2
Q

what does a high and positive electrode potential mean?

A

very good oxidising agent

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3
Q

what is the emf of a standard hydrogen electrode?

A

0

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4
Q

why is the emf of the she 0?

A

acts as a baseline - used as a comparison

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5
Q

how should the standard hydrogen electrode and the other half cell be connected?

A

with a high resistance voltmeter and a salt bridge

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6
Q

how can you make a salt bridge?

A

soak filter paper in potassium chloride/nitrate

fill a u tube with KCl in agar jelly

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7
Q

what is the purpose of a salt bridge?

A

completes the circuit

balances the charges

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8
Q

why do you stopper the end of a salt bridge with cotton wool?

A

to stop too much mixing of salt bridge solution with the contents of the two beakers

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9
Q

describe how the standard hydrogen electrode is set up

A

solution of H+ ions
platinum electrode (platinum foil over porous platinum)
H2 gas

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10
Q

what standard conditions are all half cells under?

A

all solutions are 1M
gases at 100kPa
298K temp

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11
Q

why do half cells need to be under standard conditions?

A

because the equilibrium shifts with a change in conditions

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12
Q

why is a high resistance voltmeter needed when connecting two half cells?

A

to avoid the flow of current because this will cause a drop in the voltage

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13
Q

define standard electrode potential

A

the electrode potential of a standard electrode with ion conc of 1M at 298K connected to a standard H electrode using a high resistance voltmeter and salt bridge

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14
Q

which side does the oxidation half cell go on?

A

the left

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15
Q

which side does the reduction electrode go on?

A

the right

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16
Q

what is the equation to find the EMF of a whole cell?

A

E(rhs)-E(lhs)

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17
Q

explain how electrode potentials can show the feasability of a cell?

A

the more positive a cell’s emf, the more feasible the reaction

18
Q

which side is the SHE always on?

19
Q

give a commercial use of cells

A

commercial source of electrical energy

20
Q

what are primary cells?

A

single use/disposable cells

21
Q

what are secondary cells?

A

rechargeable cells

22
Q

what’s an example of a non-rechargeable cell?

A

Zn and MnO2

23
Q

advantages of non-rechargeable cells

A

low cost

non-toxic material

24
Q

disadvantages of non-rechargeable cells

A

can leak
cannot be recycled
unstable

25
give examples of rechargeable cells
nickel cadmium lead-acid lithium ion
26
give some uses of lithium ion cells
provide electrical energy for tablets, laptops and phones
27
what is the purpose of graphite powder in a lithium fuel cell?
acts as a support medium
28
why can water not be used in a lithium fuel cell?
reacts with the lithium
29
give the equation of the oxidation reaction in a lithium ion cell
Li ----> Li+ + e-
30
give the equation of the reduction reaction in a lithium ion cel
e- + Li+ + CoO2 ---> Li+[CoO2]-
31
give the cell notation for a lithium ion cell
Li(s)/Li+(aq) // Li+, CoO2/ Li+[CoO2]-
32
advantages of rechargeable cells?
reusable prevents waste slows depletion of metals and other reagents less energy used to extract metals
33
what is a fuel cell?
a cell which converts chemical energy from a redox reaction into electrical energy (generate an electric current)
34
what are the main types of fuel cell?
hydrogen or ethanol
35
give the oxidation reaction in an acidic hydrogen fuel cell
H2(g) ----> 2H+(aq) + 2e-
36
give the reduction reaction in the acidic hydrogen fuel cell?
O2(g) + 4H+ + 4e- -----> 2H2O (l)
37
give the oxidation reaction in an alkaline hydrogen fuel cell
H2 + 2OH- ----> 2H2O
38
give the reduction reaction in an alkaline hydrogen fuel cell
O2 (g) + 2H2O + 4e- ----> 4OH-
39
what are the advantages of fuel cells?
no need to recharge them run for as long as you supply them with fuel steady output of voltage doesn't generate CO2 - only product is water
40
what is the advantage of using fuel cells in cars?
uses more available energy for kinetic energy so less energy is wasted as heat
41
what are the disadvantages of fuel cells?
not carbon neutral bc CO2 released when the methane and steam react to form hydrogen expensive difficult to store flammable