Final answer:
To calculate the grams of quicklime produced, use stoichiometry. Convert the mass of limestone to moles, then convert moles of CaO to grams.
Step-by-step explanation:
To calculate how many grams of quicklime (CaO) can be produced from 2.0 kg of limestone (CaCO3), we need to use stoichiometry, which is a way of calculating the quantities of reactants and products in a chemical reaction. The balanced equation for the decomposition of limestone is:
CaCO3(s) → CaO(s) + CO2(g)
From the equation, we can see that one mole of CaCO3 produces one mole of CaO. To convert from grams to moles, we need to use the molar mass of CaCO3, which is 100.09 g/mol.
First, convert the mass of limestone to moles:
2.0 kg × (1000 g/1 kg) ÷ (100.09 g/mol) = 19.98 mol
Therefore, 2.0 kg of limestone can produce 19.98 moles of quicklime. Since one mole of CaCO3 produces one mole of CaO, 19.98 moles of CaCO3 produces 19.98 moles of CaO.
Finally, convert moles of CaO to grams:
19.98 mol × 56.08 g/mol = 1119.64 g
Therefore, approximately 1119.64 grams of quicklime can be produced from 2.0 kg of limestone.