Final answer:
The balanced equation for the redox reaction MnO4- + I- + H+ → Mn2+ + I2 + H2O in acidic solution is 2 MnO4- + 10 I- + 16 H+ → 2 Mn2+ + 5 I2 + 8 H2O, reflecting the conservation of mass and charge.
Step-by-step explanation:
The student appears to be asking about how to balance a redox reaction equation. In the given unbalanced chemical equation, MnO4- is reduced to Mn2+, and I- is oxidized to I2. It is necessary to balance both the atoms and the charges to ensure that the mass and charge are conserved across the equation. Typically, the charges are balanced by adding H+ ions in acidic solution or OH- ions in basic solution. The addition of water molecules (H2O) is used to balance oxygen atoms. Balancing everything, including the atoms (Mn, I, O, and H), the charges, and ensuring the electrons transferred in the oxidation and reduction are equal, gives us the balanced equation:
2 MnO4- + 10 I- + 16 H+ → 2 Mn2+ + 5 I2 + 8 H2O
This equation represents complete atom and charge balance in an acidic solution, indicating that 2 moles of permanganate ions react with 10 moles of iodide ions and 16 moles of hydrogen ions to produce 2 moles of manganese(II) ions, 5 moles of iodine molecules, and 8 moles of water.