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C4 - Mocks - Coggle Diagram
C4 - Mocks
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C5 - Mocks
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L3 - Simple Cells
A simple cell is constructed using two different metal electrodes, these electrodes differ in reactivity. The larger the difference in reactivity, the greater the potential difference.
In non-rechargeable batteries (alkaline batteries) the reaction stops when one of the reactants is used up, the reaction is not reversible.
L4 - Fuel Cells
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In hydrogen fuel cells, hydrogen is oxidised electrochemically to produce water and a potential difference.
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Pros: Only water produced, relatively simple devices, last longer than batteries, only require hydrogen and oxygen.
Cons: Require more space to store, hydrogen is flammable, expensive, lack of infrastructure.
L5 - The pH Scale
All acids contain H+ ions, all alkalis contain OH- ions.
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L9 - Electrolysis Pt2
Aluminium is a lightweight, non-corrosive metal; it is a good thermal and electrical conductor that is found naturally as bauxite.
During the electrolysis of aluminium oxide, oxygen reacts with the anode to produce carbon dioxide, this means that the anode had to be regularly replaced.
Cryolite is used to lower the melting point of a substance, this makes the process more economically viable.
L8 - Electrolysis Pt1
During the electrolysis of a molten ionic compounds, oxidation takes place at the anode; this is because the non-metal ions lose electrons here. Reduction takes place at the cathode because positive metal ions gain electrons here.
During electrolysis of a molten ionic compound, a solid or molten metal will form at the cathode. A halide gas may be produced as the anode.
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L2 - Reactivity Series
Elements under hydrogen:
- Copper
- Mercury
- Silver
- Gold
- Platinum
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