Final answer:
To balance the given redox reaction in acidic solution, the permanganate ion reduction and zinc oxidation half-reactions are balanced separately and then combined. The final balanced equation is 16H+ + 2MnO4- + 5Zn → 2Mn2+ + 5Zn2+ + 8H2O.
Step-by-step explanation:
The student's question involves the balancing of a redox reaction in acidic solution. The half-reactions for this equation must be balanced separately for mass and charge before combining them back together to form the overall balanced equation.
For the reduction half-reaction involving permanganate ion (MnO4−):
8H+ + MnO4− + 5e− → Mn2+ + 4H2O
For the oxidation half-reaction involving zinc (Zn):
Zn → Zn2+ + 2e−
To balance the charges, multiply the oxidation half-reaction by 5 and the reduction half-reaction by 2, and then add them together:
16H+ + 2MnO4− + 5Zn → 2Mn2+ + 5Zn2+ + 8H2O
The redox reaction is now balanced in terms of both mass and charge.