Non rechargeable cells: function of carbon rod
Key Terms
Rechargeable cells: examples
lead/acid- cars
Ni/Cd- torches/radios
lithium/ion-phones, tablets, cameras etc
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| Term | Definition |
|---|---|
Non rechargeable cells: function of carbon rod | Allows electrons to flow |
Non rechargeable cells: why cell often leaks after being used for a long time | Zn used up as reaction proceeds |
Rechargeable cells: why can they be recharged | Reaction occurring in cell can be reversed and chemicals in cell regenerated |
Rechargeable cells: examples |
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Lithium ion cells: why are they light | Lithium is the least dense mental |
Lithium ion cells: reaction occurring at positive electrode | Co(IV) reduced to Co(III) |
Lithium ion cells: reaction occurring at negative electrode | Li(0) oxidised to Li(+1) |
Lithium ion cells: equation for discharge of cell | CoO2 + Li > Li+[CoO2]- |
Lithium ion cells: equation for recharging cell | Discharge reaction reversed | Li+[CoO2]- > CoO2 + Li |
The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Cu2+]<1moldm-3 |
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The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Zn2+]>1mol dm-3 |
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The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Zn2+] < 1moldm-3 |
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if conditions are no longer standard what is cell potential written as as opposed to E0Cell | ECell |
Limitations of using electrode potentials to predict redox reactions | predictions using electrode potentials tell us about equilibrium but not RoR many reactions in laboratory not done under standard conditions- will affect electrode potential vales |
Commercial applications of electrochemical cells: what 3 main types can cells be divided into |
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Non rechargeable cells: how are they designed to be used only once | Reactions occurring in cells cannot be reversed |
Non rechargeable cells: what will happen when the chemicals are used up | The battery will go flat and the emf will fall to 0.00V |
Non rechargeable cells: used in | Smoke detectors and clocks |
Non rechargeable cells: overall equation of zinc and manganese dioxide cell when it discharged | 2MnO2 + 2H2O + Zn > 2MnO(OH) + 2OH- + Zn2+ |
Non rechargeable cells: function of porous separator | Allows ions to flow |
Non rechargeable cells: function of carbon rod | Allows electrons to flow |
Non rechargeable cells: why cell often leaks after being used for a long time | Zn used up as reaction proceeds |
Rechargeable cells: why can they be recharged | Reaction occurring in cell can be reversed and chemicals in cell regenerated |
Rechargeable cells: examples |
|
Lithium ion cells: why are they light | Lithium is the least dense mental |
Lithium ion cells: reaction occurring at positive electrode | Co(IV) reduced to Co(III) |
Lithium ion cells: reaction occurring at negative electrode | Li(0) oxidised to Li(+1) |
Lithium ion cells: equation for discharge of cell | CoO2 + Li > Li+[CoO2]- |
Lithium ion cells: equation for recharging cell | Discharge reaction reversed | Li+[CoO2]- > CoO2 + Li |
Fuel cells: what does it use to create a voltage | Energy from the reaction of a fuel with oxygen |