Chemestry Problems... Balance the following redox reaction in acidic solution: ..?

One problem is in acidic, the other is in basic...not sure what the formula difference is...

1. Balance the following redox reaction in acidic solution:
HClO2 + MnO2 -- Cl2 + MnO4-

2.Balance the following redox reaction in basic solution?

Cl2O7 (g) + H2O2 (aq) -- ClO2- (aq) + O2 (aq)

Answer:
In the first one your half reactions are:

6 H+ + 6 e- + 2 HClO2 = Cl2 + 4 H2O
MnO2 + 2 H2O = MnO4(-) + 4 H+ + 3 e-

Multiply the second equation through by 2 and then add up

Now listen .. balancing in base is easy. What you do is just balance it in acid, and then add enough OH(-) to the side that has the H(+) to convert it all to water. After all, H(+) + OH(-) = H2O. Everyone knows that! Then cancel the extra waters on either side.

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