1. what voltage is necessary to force the following electrolysis reaction to occur? which process would occur at the anode? cathode? assuming the iodine oxidation takes place at a platinumm electrode, what is the direction of electron flow in this cell? 2I^(-)(aq)+Cu^(+2)(aq)---I2(s)+Cu(s)

Question

1. what voltage is necessary to force the following electrolysis reaction to occur? which process would occur at the anode? cathode? assuming the iodine oxidation takes place at a platinumm electrode, what is the direction of electron flow in this cell?  2I^(-)(aq)+Cu^(+2)(aq)--->I2(s)+Cu(s)

DrBob222 · Answer

I don't know what you're asking. For b, you want to know anode and cathode for which reaction? The spontaneous or non-spontaneous cell.

For the cell given, look up each half reaction and calculate the Ecell. If it is +, the reaction proceeds as written and the anode is where oxidation occurs.