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)
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.
To determine the voltage necessary for the electrolysis reaction, we need to consider the standard electrode potentials (E°) of the half-reactions involved.
First, let's write the half-reactions for the anode and cathode:
At the anode, I^(-)(aq) undergoes oxidation to form I2(s):
2I^(-)(aq) → I2(s) + 2e^-
This half-reaction involves the loss of electrons and occurs at the anode.
At the cathode, Cu^(+2)(aq) undergoes reduction to form Cu(s):
Cu^(+2)(aq) + 2e^- → Cu(s)
This half-reaction involves the gain of electrons and occurs at the cathode.
Next, let's refer to a standard electrode potential table to determine the standard electrode potentials for each half-reaction. The more positive the standard electrode potential, the easier it is for the reaction to occur.
The standard electrode potential for the reduction of Cu^(+2)(aq) to Cu(s) is +0.34 V, and the standard electrode potential for the oxidation of I^(-)(aq) to I2(s) is +0.54 V.
To calculate the overall voltage required for the reaction, we subtract the standard electrode potential of the anode reaction (oxidation) from the standard electrode potential of the cathode reaction (reduction):
E°cell = E°cathode - E°anode = 0.34 V - 0.54 V = -0.20 V
The negative value indicates that the reaction is not spontaneous under standard conditions, so an external voltage is required to force the reaction to occur.
To determine the direction of electron flow in this cell, we can use the mnemonic "AN OX" (Anode Oxidation) and "RED CAT" (Reduction Cathode) to remember that oxidation occurs at the anode and reduction occurs at the cathode.
So, in this cell setup, electrons will flow from the I^(-)(aq) at the anode towards the Cu^(+2)(aq) at the cathode.
Therefore, the voltage necessary to force this electrolysis reaction to occur is a minimum of 0.20 V, and the process of iodine oxidation occurs at the anode while copper reduction occurs at the cathode.