Final answer:
The redox reaction Zn(s) + H2O(l) → Zn2+(aq) + H2(g) is balanced in a basic solution by writing the oxidation and reduction half-reactions, balancing them for mass and charge, combining them to cancel electrons, and making final adjustments to balance oxygen and hydrogen.
Step-by-step explanation:
To balance the given redox reaction Zn(s) + H2O(l) → Zn2+(aq) + H2(g) in a basic solution, we need to follow the half-reaction method:
- Write the oxidation and reduction half-reactions. Zinc is oxidized:
- Balance the half-reactions for mass and charge. In basic solutions, add OH− to balance H+ if present.
- Combine the two balanced half-reactions, ensuring that the electrons cancel out.
- Make final adjustments to balance the oxygen by adding H2O as needed and balance hydrogen by adding OH− ions.
The balanced redox reaction is:
Zn(s) + 4 OH− (aq) → Zn2+(aq) + 2 H2O(l) + 2e− (1)
Hydrogen is produced at the cathode:
2e− + 2 H2O(l) → H2(g) + 2 OH− (aq) (2)
Adding both half-reactions (1) and (2) together gives us the balanced reaction:
Zn(s) + 2 H2O(l) → Zn2+(aq) + H2(g) + 2 OH− (aq)