Calcium carbonate (CaCO3 ) can undergo a chemical reaction to produce calcium oxide (CaO ) and carbon dioxide (CO2 ). Which possible masses of calcium oxide and carbon dioxide can form when 200g of calcium carbonate undergoes this chemical reaction?(1 point) Responses 40g CaO and 12g CO2 40g cap c A cap o and 12g cap c cap o sub 2 200g CaO and 200g CO2 200g cap c A cap o and 200g cap c cap o sub 2 112g CaO and 88g CO2 112g cap c A cap o and 88g cap c cap o sub 2 56g CaO and 44g CO2
112g CaO and 88g CO2
To find the masses of each product formed, we first need to determine the molar ratios between calcium carbonate, calcium oxide, and carbon dioxide in the balanced chemical equation. The balanced chemical equation for the reaction is:
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 each compound:
- CaCO3: 40.08 (Ca) + 12.01 (C) + 3(16.00) (O) = 100.09 g/mol
- CaO: 40.08 (Ca) + 16.00 (O) = 56.08 g/mol
- CO2: 12.01 (C) + 2(16.00) (O) = 44.01 g/mol
Now we can calculate the theoretical yield of each product:
- For CaO: (200g CaCO3) * (1 mol CaCO3 / 100.09g CaCO3) * (1 mol CaO / 1 mol CaCO3) * (56.08g CaO / 1 mol CaO) = 112g CaO
- For CO2: (200g CaCO3) * (1 mol CaCO3 / 100.09g CaCO3) * (1 mol CO2 / 1 mol CaCO3) * (44.01g CO2 / 1 mol CO2) = 88g CO2
Therefore, the possible masses of calcium oxide and carbon dioxide that can form when 200g of calcium carbonate undergoes this chemical reaction are 112g CaO and 88g CO2.