split the following redox equation to oxidation and reduction
1 Fe 2Ag -> Fe2 2Ag
2 Cl2 I -> 2Cl- I2?
Not very well posted.
Oxidation is the loss of electrons. Reduction is the gain of electrons.
Fe ==> Fe^2+ + 2e
2Ag to 2Ag isn't right. It should be 2Ag^+ + 2e ==> 2Ag
Sure! To identify the oxidation and reduction in a redox equation, you need to determine the changes in oxidation numbers of the elements involved.
Let's break down each equation:
1) Fe + 2Ag -> Fe2 + 2Ag
To determine the oxidation and reduction, you need to identify the element that is getting oxidized and the element that is getting reduced.
In this equation, the iron (Fe) is being oxidized because its oxidation state increases from 0 to +2. The silver (Ag) is being reduced because its oxidation state decreases from 0 to 0.
So, the oxidation half-reaction is:
Fe -> Fe2+ (+2e-)
And the reduction half-reaction is:
2Ag+ (+2e-) -> 2Ag
2) Cl2 + 2I -> 2Cl- + I2
Again, let's identify the oxidized and reduced elements.
In this equation, the chlorine (Cl) is being reduced. Its oxidation state decreases from 0 to -1. The iodine (I) is being oxidized as its oxidation state increases from 0 to 0.
So, the oxidation half-reaction is:
2I- -> I2 (+2e-)
And the reduction half-reaction is:
Cl2 + 2e- -> 2Cl-
By breaking down the redox equations and identifying the changes in the oxidation numbers, we can determine the oxidation and reduction half-reactions.