How many grams of CO2 are evolved on heating 200 g of CaCO3.
? gms CO2 from decomposition of 200 gms of CaCO3.
CaCO3 => CaO + CO2
moles CaCO3 = (200g/100g/mol) = 2 mol
2mol(CO2) => 2mol(CaO) + 2mol(CO2)
2mol(CO2) = 2mol(CO2)(44g/mol) = 88gms CO2.
To find the number of grams of CO2 evolved on heating 200 g of CaCO3, we need to use the molar masses of CaCO3 and CO2, along with the balanced chemical equation.
Step 1: Write the balanced chemical equation for the reaction:
CaCO3(s) -> CaO(s) + CO2(g)
Step 2: Find the molar mass of CaCO3 and CO2:
Molar mass of CaCO3 = (1 atom of Ca x atomic mass of Ca) + (1 atom of C x atomic mass of C) + (3 atoms of O x atomic mass of O)
= (1 x 40.08 g/mol) + (1 x 12.01 g/mol) + (3 x 16.00 g/mol)
= 40.08 + 12.01 + 48.00
= 100.09 g/mol
Molar mass of CO2 = (1 atom of C x atomic mass of C) + (2 atoms of O x atomic mass of O)
= (1 x 12.01 g/mol) + (2 x 16.00 g/mol)
= 12.01 + 32.00
= 44.01 g/mol
Step 3: Calculate the number of moles of CaCO3:
Number of moles = Mass / Molar mass
= 200 g / 100.09 g/mol
= 1.999 moles (rounding to 3 significant figures)
Step 4: Determine the molar ratio between CaCO3 and CO2 from the balanced equation:
From the balanced equation, we can see that 1 mole of CaCO3 will produce 1 mole of CO2.
Step 5: Calculate the number of moles of CO2 produced:
Number of moles of CO2 = Number of moles of CaCO3
= 1.999 moles
Step 6: Convert moles to grams using the molar mass of CO2:
Mass of CO2 = Number of moles x Molar mass of CO2
= 1.999 moles x 44.01 g/mol
= 87.982 g
Therefore, approximately 88 grams of CO2 are evolved on heating 200 g of CaCO3.