Cells Flashcards

1
Q

Primary cells

A

Cells that are Not rechargeable and will eventually run out when reactants get used up

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2
Q

Secondary cells

A

Rechargeable cells that use a reversible reaction

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3
Q

What is the theory behind electrochemical cells?

A

There is a transfer of electrons in the redox reaction between half cells which acts as an electric current

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4
Q

Storage cells

A

A rechargeable cell

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5
Q

Example of a primary cell

A

Alkaline batteries: Zinc + Manganate (IV)

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6
Q

Why can Storage cells be recharged?

A

Because the overall reaction is reversible

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7
Q

Why can a current occur in an electrochemical cell?

A

Because the voltmeter was replaced with an ammeter to allow flow of electrons between half cells so overall, reactions occur

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8
Q

Why does the current in a non rechargeable cell eventually fall to 0?

A

Because the reactants get used up and form products of overall reaction
So no current will flow as no more electrons are transferred

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9
Q

What is the discharge reaction in an electrochemical cell?

A

The forward overall reaction because charge is given out when electrons from oxidised reactant is transferred to reduced reactant

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10
Q

What is the charging reaction in an electrochemical cell?

A

The backward reaction because reactants are reformed for the forward reaction to proceed again and give off more charge

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11
Q

Why do chargeable cells eventually run out of charge?

A

Because of leakage of the electrolyte solvent or side reactions occur that decrease concentration of reactants over time

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12
Q

Example of rechargeable secondary cell?

A

Lithium ion batteries

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13
Q

Why is graphite used in lithium ion batteries?

A

Because absorbs reagents so allows ions to react in absence of a solvent

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14
Q

Why can water not be used as a solvent in lithium ion batteries

A

Because it is not inert so water will react with the lithium

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15
Q

Fuel cell

A

Uses a constant supply of fuel and oxidising agent to produce a voltage via a chemical reaction (without burning the fuel)

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16
Q

General outline of how a fuel cell works

A

Fuel reacts with oxygen
Uses energy in this to create a voltage

17
Q

Examples of fuel in a fuel cell

A

Methanol
Hydrogen

18
Q

2 types of hydrogen fuel cells

A

In acidic electrolyte conditions
In alkaline electrolyte conditions

19
Q

Summary of alkaline hydrogen fuel cell: anode

A

hydrogen fed into cell and oxidised to H+ (but combines with hydroxide ions from electrolyte) to produce water
Electrons are released from oxidation

20
Q

Equation at anode of alkaline hydrogen fuel cells

A

2H₂ + 4OH⁻ —-> 2H₂O + 4e⁻
OXIDATION OF HYDROGEN GAS

21
Q

Electrolyte in an alkaline hydrogen fuel cell

A

Potassium hydroxide

22
Q

Summary of alkaline hydrogen fuel cell: cathode

A

Oxygen is fed into cell
Accepts electrons (reduced) from circuit and reacts with water to reform hydroxide ions

23
Q

Equation at cathode of an alkaline hydrogen fuel cell

A

O₂ + 2H₂O +4e⁻ —-> 4OH⁻
REDUCTION OF OXYGEN

24
Q

Why is the reaction at the anode written as reduction when it is oxidation?

A

Because the standard notation is to write electrode equations as reduction :)

25
Q

Exchange of hydroxide ions in an alkaline hydrogen fuel cell

A

between a membrane from the positive electrode (produced from reduction of oxygen) to the negative electrode (gained after hydrogen was oxidised to

26
Q

Overall hydrogen fuel cell equation

A

2H₂ + O₂ —–> 2H₂O

27
Q

Summary of acid hydrogen fuel cell: anode

A

Hydrogen is fed into the fuel cell
Hydrogen is oxidised by losing electrons to form H+ and releases electron

27
Q

Equation for the hydrogen fuel cell in acidic conditions

A

H₂ —–> 2H⁺ + 2e-

28
Q

Summary of acid hydrogen fuel cell: cathode

A

Oxygen is fed into the fuel cell and combines with H+ (from the anode) to produce water
Accepts electrons from the anode

29
Q

Electrolyte used in acid hydrogen fuel cell

A

Phosphoric acid

30
Q

How many electrons are transported in each half cell in a fuel cell?

31
Q

Why do fuel cells maintain a constant voltage over time?

A

Continuously feeding the fuel cell with H2 and O2 to maintain concentration
So concentrations of reactant remains constant over time

32
Q

Can reactions in the hydrogen fuel occur under standard conditions?

A

No, rate is too slow because the activation energy is too high

33
Q

Increasing temperature of a hydrogen fuel cell

A

Too high shifts position of equilibrium to prefer the backward endothermic reaction to take energy in so EMF falls

34
Q

How can hydrogen be stored?

A

As a liquid under pressure
Adsorbed on the surface of a solid
Absorbed on solid surface material

35
Q

Catalysts in a hydrogen fuel cell

A

Used to lower activation energy to provide an alternative reaction pathway so reaction can actually occur