posted by Angelo09 .
The following redox equation occurs in acidic aqueous solution. When it is balanced with the smallest whole number coefficients, what is the coefficient for chlorine gas?
KMnO4(aq) + KCl(aq) + H2SO4(aq) = MnSO4(aq) + K2SO4(aq) + Cl2(g)
I'm not going to balance this thing and give you the answer. This will get you started.
Mn goes from oxidation state of +7 on the left to +2 on the right.
Cl goes from -1 on the left to zero on the right (for each Cl atom/ion).
Hint: Temporarily balance the Cl atoms by placing a 2 in front of KCl and figure the electron change for two Cl^- going to Cl2. You may or may not need to change this two later.
If you are lost with this, tell us what your problem is and we can help you through it. You need to learn how to do these yourself.
I have a Chemistry test coming up this Friday with 30 Multiple Choice. It's going to be mostly calculative problems from 11 chapters. I'm just not quite sure how my approach to studying should be. Can you give me any tips? Much appreciated, thanks.
Here is a very good site that takes you through determining the oxidation state of elements (alone and in compounds) as well as how to write the half reactions and how to balance the complete equation.
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