How many moles of limestone will he required produce 5.6g of CaO?

To determine the number of moles of limestone needed to produce 5.6g of CaO, we need to use stoichiometry and the molar mass of CaO and limestone. The balanced chemical equation for the thermal decomposition of limestone is: CaCO3 (s) → CaO (s) + CO2 (g) From the equation, we can see that 1 mole of CaCO3 produces 1 mole of CaO. The molar mass of CaO is 56.077 g/mol, while the molar mass of CaCO3 is 100.0869 g/mol. To find the number of moles of CaO produced from 5.6g of CaO, we divide the mass by the molar mass: moles of CaO = mass of CaO / molar mass of CaO moles of CaO = 5.6 g / 56.077 g/mol moles of CaO = 0.1 mol Since 1 mole of CaCO3 produces 1 mole of CaO, we need 0.1 mol of CaCO3 to produce 0.1 mol of CaO. Therefore, the answer is 0.10 mol. Hence, the correct option is: - 0.10 mol