You're asking about the decomposition of lead(II) carbonate (PbCO₃) to produce lead(II) oxide (PbO) and carbon dioxide (CO₂). Here's how to solve the problem:

1. Write the Balanced Chemical Equation:

PbCO₃(s) → PbO(s) + CO₂(g)

2. Calculate the Molar Masses:

* PbCO₃: 207.2 g/mol (Pb) + 12.01 g/mol (C) + 3 * 16.00 g/mol (O) = 267.21 g/mol

* PbO: 207.2 g/mol (Pb) + 16.00 g/mol (O) = 223.2 g/mol

3. Use Stoichiometry to Find the Mass of PbO:

* Convert grams of PbCO₃ to moles:

2.50 g PbCO₃ * (1 mol PbCO₃ / 267.21 g PbCO₃) = 0.00936 mol PbCO₃

* Use the mole ratio from the balanced equation:

1 mol PbCO₃ : 1 mol PbO

Therefore, 0.00936 mol PbCO₃ will produce 0.00936 mol PbO.

* Convert moles of PbO to grams:

0.00936 mol PbO * (223.2 g PbO / 1 mol PbO) = 2.09 g PbO

Answer: 2.09 grams of lead(II) oxide will be produced by the decomposition of 2.50 grams of lead(II) carbonate.