chemistry
posted by princess .
MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced)
i. Write the reduction and oxidation halfreactions (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 halfreactions. (.5 point)
v. Multiply each halfreaction 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 halfreactions 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)

See your other post.