Can I2 oxidize metallic aluminum? Show the balanced chemical equation and the Eo values.
To determine if I2 can oxidize metallic aluminum, we need to compare the standard reduction potentials (E°) of the two species involved - I2 and Al.
The reduction half-reaction for iodine (I2) can be represented as follows:
I2 + 2e- → 2I- E° = +0.54 V
The oxidation half-reaction for aluminum (Al) can be represented as:
Al → Al3+ + 3e- E° = -1.66 V
In this case, we can see that the reduction potential of I2 is higher (+0.54 V) than that of Al (-1.66 V). According to the electrochemical series, a higher reduction potential indicates a stronger oxidizing agent.
Therefore, I2 is strong enough to oxidize Al.
Now, let's write the balanced chemical equation for this reaction:
2 I2 + 6 Al → 6 Al3+ + 4 I-
Please note that this is an unbalanced equation. To balance the equation, we need to ensure that the number of atoms on each side is equal:
3 I2 + 6 Al → 6 Al3+ + 2 I-
So, to summarize:
I2 can oxidize metallic aluminum, as shown by the balanced chemical equation:
3 I2 + 6 Al → 6 Al3+ + 2 I-
And the E° values for the half-reactions involved are:
I2 reduction: E° = +0.54 V
Al oxidation: E° = -1.66 V