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Electrolysis of copper sulphate solution?
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Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):
Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu
I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)
Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu
I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)
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#4
(Original post by surina16)
AQA last topic of C2? (we're so behind arghhhh)
AQA last topic of C2? (we're so behind arghhhh)
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#7
(Original post by surina16)
Mayhem™
For higher tier: "Candidates should be able to complete andbalance half equations for the reactions occurring at the electrodes during electrolysis."
Mayhem™
For higher tier: "Candidates should be able to complete andbalance half equations for the reactions occurring at the electrodes during electrolysis."
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wanted to check that the stuff we're learning is actually relevant :/
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#9
(Original post by surina16)
Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):
Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu
I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)
Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):
Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu
I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)
This is deffo on the AQA papers. Just remember that the Anodes positive, The Cathode is negative then remember the products. There's no explanation, just gotta learn it
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(Original post by Her._.Majesty)
This is deffo on the AQA papers. Just remember that the Anodes positive, The Cathode is negative then remember the products. There's no explanation, just gotta learn it
This is deffo on the AQA papers. Just remember that the Anodes positive, The Cathode is negative then remember the products. There's no explanation, just gotta learn it
Yeah we have the acronym PANIC to remember it
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#12
(Original post by surina16)
Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):
Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu
I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)
Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):
Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu
I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)
The negative sulphate ions (SO42-) or the traces of hydroxide ions (OH–) are attracted to the positive electrode. But the sulfate ion is too stable and nothing happens. Instead either hydroxide ions or water molecules are discharged and oxidised to form oxygen.
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#13
(Original post by hxfsxh)
During electrolysis:the cathode gets coated with copper. bubbles of oxygen are given off at the anode As the copper ions are discharged as copper atoms at the cathode, the blue colour of the solution gradually fades and an oxidation reaction occurs which is the 4e- (electron loss).
The negative sulphate ions (SO42-) or the traces of hydroxide ions (OH–) are attracted to the positive electrode. But the sulfate ion is too stable and nothing happens. Instead either hydroxide ions or water molecules are discharged and oxidised to form oxygen.
During electrolysis:the cathode gets coated with copper. bubbles of oxygen are given off at the anode As the copper ions are discharged as copper atoms at the cathode, the blue colour of the solution gradually fades and an oxidation reaction occurs which is the 4e- (electron loss).
The negative sulphate ions (SO42-) or the traces of hydroxide ions (OH–) are attracted to the positive electrode. But the sulfate ion is too stable and nothing happens. Instead either hydroxide ions or water molecules are discharged and oxidised to form oxygen.
if the positive ion is above hydrogen in the reactivity series then hydrogen is formed
this applies to substances in aqueous solution ONLY.this rule doesn't apply to molten substances
just an additional info
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