I need steps of solving this question

Balance the oxidation reduction equation in electron ion / half reaction
PbO2 + KCL = KCLO + KPb(OH)3
please
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To balance the oxidation-reduction (redox) equation, you need to follow these steps:

Step 1: Assign oxidation numbers.
Start by assigning oxidation numbers to each element in the equation. The oxidation number is a positive or negative number that represents the charge an atom would have if electrons were transferred completely. Here are the oxidation numbers for each element in the equation:
Pb: +4 (since it is in the compound PbO2)
Cl: -1 (since it is in the compound KCl)
O: -2 (since it is in the compounds PbO2 and KPb(OH)3)
K: +1 (since it is in the compounds KCl and KCLO)
H: +1 (since it is in the compound KPb(OH)3)

Step 2: Identify the atoms undergoing oxidation and reduction.
In this equation, Pb is being reduced from +4 to +2, while Cl is being oxidized from -1 to 0.

Step 3: Write separate half-reactions.
Separate the redox equation into two half-reactions: one for the oxidation and another for the reduction.

Oxidation half-reaction:
Cl → ClO

Reduction half-reaction:
Pb4+ → Pb2+

Step 4: Balance atoms other than oxygen and hydrogen.
Start by balancing atoms other than oxygen and hydrogen in each half-reaction. For the reduction half-reaction, balancing the Pb atoms results in the equation:
Pb4+ → Pb2+

Step 5: Balance oxygen atoms.
Add water (H2O) molecules to balance the oxygen atoms in both half-reactions. In this case, you'll only need to balance the oxygen atoms in the reduction half-reaction. Balancing the oxygens gives:
Pb4+ → Pb2+ + 2H2O

Step 6: Balance hydrogen atoms.
Add hydrogen ions (H+) to balance the hydrogen atoms in each half-reaction. In this case, you only need to balance the hydrogen atoms in the oxidation half-reaction. Balancing the hydrogens gives:
Cl + H2O → ClO + 2H+

Step 7: Balance charges by adding electrons.
Add the appropriate number of electrons (e-) to balance the charges on both sides of each half-reaction. In this case, the reduction half-reaction will need electrons added, so it becomes:
Pb4+ + 2e- → Pb2+

Step 8: Multiply the half-reactions.
To make the number of electrons on each side equal, multiply both half-reactions by the necessary factor. In this case, you need to multiply the oxidation half-reaction by 2:
2Cl + 2H2O → 2ClO + 4H+

Step 9: Combine the half-reactions.
Now combine the two half-reactions to eliminate the electrons and form a balanced equation. In this case, the electrons cancel out, resulting in the balanced redox equation:
2Cl + 2H2O + Pb4+ → 2ClO + 4H+ + Pb2+

And that's the balanced oxidation-reduction (redox) equation for PbO2 + KCl = KCLO + KPb(OH)3.