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D) Physics > Battery Design > Flashcards

Battery Design Flashcards

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0
Q

Zinc battery reaction

A 
Do not contain high volumes of liquid
Anode Zn(s)→Zn+2(aq)+2e-
Cathode 2MnO2(s)+2NH4+(aq)+2e-→Mn2O3(s)+2NH3(g)+H2O(l)
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1
Q

Battery types

A 
Lead-Acid
Dry-cell (Alkaline and Zinc)
Nickel-Cadium (NiCad)
Nickel-Metal Hydride (NiMH)
Lithium Ion
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2
Q

Alkaline Batteries

A 
Slightly different reaction from standard zinc batteries
Anode Zn(s)+2OH-(aq)→Zn(OH)2(s)+2e-
Cathode 2MnO2(s)+2H2O(l)+2e-→Mn2O3(s)+2OH-(aq)

Overall Reaction Zn(s)+2MnO2(s)+2H2O(l)→Zn(OH)2(s)+2MnO(OH)(s)

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3
Q

Electrochemical Cell

A

A device that stages redox reaction that either results in or is driven by an electric current

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4
Q

Voltaic Cell

A

The half-cell battery component that produces the electric current from its spontaneous chemical reaction

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5
Q

Electrolytic Cell

A

The half-cell battery component that consumes current to drive its non-spontaneous chemical reaction

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6
Q

Half-cell

A

The first of two reactions in an electrochemical cell

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7
Q

Electrodes

A

Conductive surfaces through which electrons can either enter or leave the half sells

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8
Q

Electric Potential Difference

A

The difference in potential energy per unit of charge

Drives the electric current
Given in Voltage (V)

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9
Q

Cell potential (E.cell)

A

The total voltage between the two half-cells,

Depends on the relative tendencies of the reactants to undergo oxidation or reduction

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10
Q

Standard cell potential

A

Cell potential (E.cell) for 1M concentration of reactants and products in a chemical equation

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11
Q

Anode

A

The voltaic half-cell in which oxidation occurs from a spontaneous reaction
Gives an electron in products
Denoted (-) on the battery surface

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12
Q

Cathode

A

The electrolytic Half-cell that undergoes reduction
Consumes an electron to drive the non-spontaneous reaction
Denoted (+) on the battery surface

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13
Q

Standard electrode potential

A

The potential of an individual electrode in a halfcell

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14
Q

‘Salt bridge’

A

The battery component that supplies both the anode and the cathode with electrolytes to help fuel the reaction

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15
Q

Standard Hydrogen Electrode

A

The half-cell electrode that is normally chosen to have a potential of zero

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16
Q

Determining current direction

A

From the anode to the cathode, always

Determine which reaction undergoes oxidation, thats the anode, where the current is produced

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17
Q

Faradays constant

A

96,485

18
Q

Electrolysis

A

The process through which an electric current passes through the cathode to drive its non-spontaneous reaction

19
Q

Dry Cell Batteries

A

Batteries in which neither the anode nor the cathode contains high volumes of liquid reactants

20
Q

Lithium ion battery mechanism of action

A

Lithium ions naturally travel from graphite to a (transition metal)-oxide, forming Lithium (transition metal)-oxide and producing a charge
The recharge uses an electric current to strip the lithium ions from the cathode

21
Q

Nickel metal-Hydride reaction mechanism

A

Anode M,H(s)+OH-(aq)→M,(s)+H2O(l)+e-
Where ‘M,’ indicates a metal alloy
Cathode NiO(OH)(s)+H2O(l)+e-→Ni(OH)2(s)+OH-(aq)

22
Q

Nickel-cadmium battery mechanism of action

A 
Anode Cd(s)+2OH-(aq)→Cd(OH)2(s)+2e-
Cathode 2NiO(OH)(s)+2H2O(l)+2e-→2Ni(OH)2(s)+2OH-(aq)
23
Q

Hydrogen Fuel Cell

A

Hydrogen gas and a hydroxide solution are supplied to the cell and react, producing water and giving off 4 electrons. These electrons run up the anode, are supplied to the electrical circuit, and re-enter the fuel cell through the cathode where they drive the reaction between oxygen gas and water producing 4OH- ions

24
Q

Alcohol based Batteries

A

Ethyl-alcohol (CH3CH2OH) gas reacts with a OH- solution in the anode,producing acetic acid gas (HC2H3O2), liquid water, and giving off 4 electrons which run through the circuit and back to the cathode to drive the reaction between oxygen gas and the water to re-form the OH- solution

25
Q

Galvanic corrosion

A

A type of corrosion that occurs when two metals are in electrical contact with one another

26
Q

Factors in galvanic corrosion

A

Humidity, anode to cathode surface area ratio, metal types, temperature, salinity

27
Q

Galvanic Serries

A

An ordered list of materials that describe (from noble to active) metals that resist galvanic corrosion

28
Q

Betavoltaic cells

A

Uses a beta-radiation to supply electrons to a system and an electrolytic cell as a cathode

29
Q

Reciprocating electromechanical atomic batteries

A

Battery builds up a difference in charge between two plates, as one approaches the other, they make contact and redistribute their charge, pushing each other appart, putting pressure on a piezoelectric material

30
Q

Optoelectric nuclear battery

A

The beta-nucleide emits beta particles that stimulate a excimer mixture, used as a photovoltaic cell

31
Q

Alpha-voltaic batteries

A

Use alpha-particles (He-4) to produce electrons from semi-conductors

32
Q

Proper battery casing

A

Plastic tube housing externally covered with a layer of aluminum

33
Q

Proper battery storage

A

Give initial charge before storing
Side by side, never with the ends touching,
At low temperatures to preserve electric potential recovery
Keep dry at all costs

34
Q

Factors in designing custom batteries

A

1) Battery life
2) Density (Weight to Volume)
3) Voltage demands
4) ‘Green’ friendly factors
5) Corrosive properties of the operating environment
6) Thermal requirements

35
Q

Homemade Battery from Soda

A

1) Pour soda in plastic cup
2) Insert a tall piece of aluminum in soda and clip to cup edge
3) Insert a tall piece of copper in soda and clip to cup edge
4) Test electrodes with the voltmeter (or circuit)

36
Q

Homemade Battery from Saltwater

A

1) Pour water in plastic cup
2) Mix tablespoon of salt
3) Clip aluminum strip to the edge
4) Clip zinc strip to the edge
5) test with a voltmeter or circuit

37
Q

Homemade battery from high molarity bleach solution

A

1) Pour water in plastic cup
2) Mix bleach
3) Clip copper strip to the edge
4) Clip aluminum strip to the edge
5) test with a voltmeter or circuit

38
Q

Homemade lemon battery

A

1) Prep the lemon by squeezing the inside without breaking the peel at all
2) Insert copper into lemon
3) Insert Steel into lemon
4) Wire up a few more, connecting ones steel to the other’s copper
5) test with voltmeter or curciut

39
Q

‘Green’ factors in batteries

A 
Galvanic corrosion products,
Nuclear Penetrating power,
Rechargeable,
Digestion effects,
Fracture Exposure effects,
Production energy,
Supply sources
40
Q

Battery Gibbs free energy

A

ΔG=-nFE.cell

F=faradays constant
n=moles

41
Q

Battery Equilibrium constant from voltage

A

log(K)=E.cell/(0.0592/n)

42
Q

Voltage from battery equilibrium

A

E.cell=(0.0592/n)*log(K)

D) Physics (13 decks)

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