Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?

• A. 2 PbO_2 ightarrow 2 PbO + O_2
• B. PbO_2 ightarrow PbO + 2 O_2
• C. 2 PbO_2 ightarrow Pb_2O_3 + O_2
• D. PbO_2 ightarrow Pb + O_2

Answer: (A)

Verified step by step guidance

1. Identify the chemical formula of lead(IV) oxide, which is \(\mathrm{PbO_2}\), indicating lead in the +4 oxidation state combined with oxygen.
2. Write the general form of the decomposition reaction where lead(IV) oxide breaks down into simpler substances, typically lead oxide and oxygen gas: \(\mathrm{PbO_2 \rightarrow \text{products}}\).
3. Balance the lead atoms on both sides of the equation. Since lead appears as \(\mathrm{Pb}\) in both reactants and products, ensure the number of lead atoms is equal.
4. Balance the oxygen atoms by adjusting coefficients so that the total number of oxygen atoms on the reactant side equals that on the product side. Remember that oxygen gas is \(\mathrm{O_2}\), so oxygen atoms must be balanced in pairs.
5. Verify that the equation is balanced in terms of both mass and charge, confirming that the number of atoms of each element is the same on both sides of the equation.