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Electrolysis

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xorichard:
OHHHHH okay thank you heaps! was confused because i was taught to split the table into half and reverse stuff and all. There's an easy question i kind of need assistance on because im dumb, it states, "For the electrolysis of a neutral nickel (II) chloride aqueous solution using inert platnium electrodes, predict the electrode reactions. Give the electrode half reactions and the overall cell reaction." Thanks again in advanced!!

RuiAce:

--- Quote from: xorichard on August 25, 2016, 05:09:11 pm ---OHHHHH okay thank you heaps! was confused because i was taught to split the table into half and reverse stuff and all. There's an easy question i kind of need assistance on because im dumb, it states, "For the electrolysis of a neutral nickel (II) chloride aqueous solution using inert platnium electrodes, predict the electrode reactions. Give the electrode half reactions and the overall cell reaction." Thanks again in advanced!!

--- End quote ---
If we are trying to decompose NiCl2 through electrolysis, it makes sense to say that the nickel ions will be reduced and the chloride ions will be oxidised.

Ni2+ + 2 e- -> Ni(s)
2 Cl- -> Cl2(g) + 2 e-

The platinum electrode exists simply to ensure the reaction happens.

Chlorine gas is the product and not aqueous solution because this is electrolysis - it will find a way to escape.

xorichard:
Thank you, boss!! Greatly appreciate your assistance today, helped me a lot! :)

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