If 3.00 mol of calcium carbonate is heated to produce calcium oxide and carbon dioxide, how many grams of calcium oxide are produced?
Follow the steps in this example.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To find the mass of calcium oxide produced, we need to use the stoichiometry of the reaction and the molar masses of calcium carbonate and calcium oxide.
Let's start by writing the balanced chemical equation for the reaction:
CaCO3(s) -> CaO(s) + CO2(g)
From the balanced equation, we can see that 1 mole of calcium carbonate (CaCO3) produces 1 mole of calcium oxide (CaO).
Given that we have 3.00 mol of calcium carbonate, we can determine the moles of calcium oxide produced.
Moles of CaO = Moles of CaCO3 = 3.00 mol
Now, we need to convert the moles of calcium oxide to grams using its molar mass. The molar mass of calcium oxide (CaO) is:
Ca: 40.08 g/mol
O: 16.00 g/mol
Molar mass of CaO = 40.08 + 16.00 = 56.08 g/mol
To find the mass of calcium oxide, we can use the following equation:
Mass of CaO = Moles of CaO × Molar mass of CaO
Mass of CaO = 3.00 mol × 56.08 g/mol
Calculating this, we find:
Mass of CaO = 168.24 grams
Therefore, 3.00 moles of calcium carbonate will produce 168.24 grams of calcium oxide.