Calcium carbonate can undergo a chemical reaction to produc calcium oxide (CaO) and carbon dioxide (CO₂). Which possible masses of calcium oxide and carbon dioxide can form when 400g of calcium carbonate undergoes this chemical reaction? * 2 points 400g CaO and 0g CO₂ 224g CaO and 176g CO₂ 40g CaO and 10g CO₂
To determine the masses of calcium oxide (CaO) and carbon dioxide (CO₂) formed when 400g of calcium carbonate undergoes this chemical reaction, we first need to write the balanced chemical equation for the reaction:
CaCO₃ → CaO + CO₂
From the equation, we can see that 1 mole of calcium carbonate produces 1 mole of calcium oxide and 1 mole of carbon dioxide.
Next, we need to calculate the molar masses of the compounds involved:
CaCO₃ = 40.08g (Ca) + 12.01g (C) + 3(16.00g) (O) = 100.09g/mol
CaO = 40.08g (Ca) + 16.00g (O) = 56.08g/mol
CO₂ = 12.01g (C) + 2(16.00g) (O) = 44.01g/mol
Now, we can calculate the number of moles of calcium carbonate present in 400g:
Number of moles = Mass / Molar mass
Number of moles of CaCO₃ = 400g / 100.09g/mol = 3.997 moles
Since the reaction stoichiometry is 1:1 for CaCO₃ to CaO and CO₂, the number of moles of CaO and CO₂ formed will also be 3.997 moles.
Finally, we can calculate the masses of CaO and CO₂ formed:
Mass of CaO = Number of moles of CaO * Molar mass of CaO
Mass of CaO = 3.997 moles * 56.08g/mol = 224g
Mass of CO₂ = Number of moles of CO₂ * Molar mass of CO₂
Mass of CO₂ = 3.997 moles * 44.01g/mol = 175.69g
Therefore, the possible masses of calcium oxide and carbon dioxide that can form when 400g of calcium carbonate undergoes this chemical reaction are approximately 224g of CaO and 176g of CO₂, which aligns with the second option provided.