Balance the following redox equation and identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent. Show all of the work used to solve the problem.

Br- + MnO2 Br2 + Mn2+

Br- + MnO2 → Br2 + Mn2+ ?
In order to balance this equation, we have to have the same number of atoms of each element of both sides. This is how to do this:
2Br− + MnO2 →Br2 + Mn + O2

Br is oxidized, because it loses electrons. Mn and O are reduced, because they gain electrons. Oxidizing agents are Mn and O, because they are reduced. And reducing agent is Br, because it is oxidized.

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Balance the following redox equation and identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent. Show all of the work used to solve the problem. Br- + MnO2 Br2 + Mn2+

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Balance the following redox equation and identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent. Show all of the work used to solve the problem.

Br- + MnO2 Br2 + Mn2+