Question

Given the half-reactions:

Cd(s) -> Cd(OH)₂ (s) oxidation half- reaction
Ni₂O₃ (s) -> Ni(OH)₂ (s) reduction half- reaction
write the balanced redox reaction (assume basic solution).

Answer 1

To construct a balanced redox reaction in a basic solution, start with writing and balancing the half-reactions for oxidation and reduction processes, balance elements, oxygen using H2O, hydrogen using OH-, and charges using electrons. Combine the balanced half-reactions to obtain the overall balanced redox reaction.

Step-by-step explanation:

To answer the question regarding the balanced redox reaction in a basic solution using the provided half-reactions for cadmium and nickel oxides, we must first correctly write and balance the half-reactions for oxidation and reduction processes.

The oxidation half-reaction is:

• Cd(s) → Cd(OH)2(s) + 2e-

The reduction half-reaction is:

• Ni2O3(s) + 2e- → 2Ni(OH)2(s)

Now, let's balance the half-reactions in a basic solution:

1. Balance all elements except hydrogen and oxygen.
2. Balance oxygen by adding H2O on the necessary side.
3. Balance hydrogen by adding OH- on the necessary side.
4. Balance the charges by adding electrons.

For example, the reduction half-reaction balance looks like this:

• Ni2O3(s) + H2O(l) + 2e- → 2Ni(OH)2(s)

Finally, once both half-reactions are balanced, they can be combined to give the overall redox reaction for the system in basic solution.