When 10.0 g of calcium carbonate (CaCO_3) is heated, what mass of carbon dioxide (CO_2) is produced?

• A. 8.8 g
• B. 2.2 g
• C. 10.0 g
• D. 4.4 g

Answer: (D)

Verified step by step guidance

1. Write the balanced chemical equation for the thermal decomposition of calcium carbonate: \(\mathrm{CaCO_3 (s) \rightarrow CaO (s) + CO_2 (g)}\).
2. Calculate the molar mass of calcium carbonate (\(\mathrm{CaCO_3}\)) by adding the atomic masses of calcium (Ca), carbon (C), and three oxygens (O): \(M_{CaCO_3} = M_{Ca} + M_C + 3 \times M_O\).
3. Calculate the molar mass of carbon dioxide (\(\mathrm{CO_2}\)) by adding the atomic masses of carbon and two oxygens: \(M_{CO_2} = M_C + 2 \times M_O\).
4. Determine the number of moles of calcium carbonate decomposed using the given mass: \(n_{CaCO_3} = \frac{\text{mass of } CaCO_3}{M_{CaCO_3}}\).
5. Use the stoichiometry of the reaction (1 mole of \(\mathrm{CaCO_3}\) produces 1 mole of \(\mathrm{CO_2}\)) to find the mass of \(\mathrm{CO_2}\) produced: \(\text{mass of } CO_2 = n_{CaCO_3} \times M_{CO_2}\).