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MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced)


i. Write the reduction and oxidation half-reactions (without electrons). (.5 point)










ii. Balance the equations for atoms (except O and H). (.5 point)










iii. Balance the equations for atoms O and H using H2O and H+. (.5 point)















iv. Balance the charge in the half-reactions. (.5 point)










v. Multiply each half-reaction by the proper number to balance charges in the reaction. (.5 point)










vi. Add the equations and simplify to get a balanced equation. (.5 point)















b. Assume a reaction takes place in a basic solution to form the given products:

MnO4–(aq) + Cl–(aq) MnO2(s) + Cl2(g) (unbalanced)


i. Balance the given half-reactions for atoms and charge. (.5 point)

MnO4– + H2O MnO2 + OH–


Cl– Cl2
















ii. Multiply to balance the charges in the reaction. (.5 point)










iii. Add the equations and simplify to get a balanced equation. (.5 point)

  • chemistry -

    I shall be happy to help you do this if you go as far as you can, then explain fully what it is you don't understand about the next step(s).

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