Electrochem/ redox Watch

beinlondon
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For the reactions I have to state the oxidiation state of each element before and after the reaction, and state whether this example is disproportionate or normal redox
2H2O(aq) -----> 2H2O(l) + O2(g)


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Veqz
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(Original post by beinlondon)
For the reactions I have to state the oxidiation state of each element before and after the reaction, and state whether this example is disproportionate or normal redox
2H2O(aq) -----> 2H2O(l) + O2(g)


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Single elements: 0
Hydrogen: +1
Oxygen: -2

Can you assign oxidation numbers now?

A disproportionate reaction is where one element is simultaneously oxidised and reduced. Can you see this looking at your oxidation numbers?
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charco
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(Original post by beinlondon)
For the reactions I have to state the oxidiation state of each element before and after the reaction, and state whether this example is disproportionate* or normal redox
2H2O**(aq) -----> 2H2O(l) + O2(g)


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Disproportionation *

H2O2 **
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