Consider the unbalanced redox reaction: MnO4-(aq) + Zn(s) → Mn2+(aq) + Zn2+(aq). Balance the equation and determine the volume of a 0.500 M KMnO4 solution required to completely react with 2.85 g of Zn.

Verified step by step guidance

1. Step 1: Identify the oxidation and reduction half-reactions. MnO4^- is reduced to Mn^2+, and Zn is oxidized to Zn^2+.
2. Step 2: Balance the atoms in each half-reaction. For the reduction half-reaction, balance Mn and then add water molecules to balance oxygen, and H+ ions to balance hydrogen. For the oxidation half-reaction, balance Zn.
3. Step 3: Balance the charges in each half-reaction by adding electrons. The reduction half-reaction will gain electrons, and the oxidation half-reaction will lose electrons.
4. Step 4: Equalize the number of electrons transferred in both half-reactions by multiplying the half-reactions by appropriate coefficients, then add the half-reactions together to get the balanced redox equation.
5. Step 5: Calculate the moles of Zn using its molar mass, then use the stoichiometry of the balanced equation to find the moles of KMnO4 needed. Finally, use the molarity of the KMnO4 solution to find the required volume.