The two half equations are
Fe^2+ ==> Fe^3+ + e
MnO4^- + 8H^+ + 5e ==> 4H2O + Mn^2+
Multiply equation 1 by 5 and equation 2 by 1 and add them. Cancel the electrons and you are left with the net ionic equation.
Use the coefficients in the balanced equation to convert 1.2E-2 mols MnO4^- to mols Fe^2+.
What is the balanced net ionic equation for the reaction between the permanganate ion and the ferrous ion in acid solution. What is the number of moles of ferrous ion that could be oxidized by 1.2×10^-2 moles of permanganate ion?
Honestly don't understand a single thing this question is asking me . All help needed!
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