How many moles of H2SO4 are required to produce 100kg of CaSO4 from CaCO3
To determine the number of moles of H2SO4 required to produce 100 kg of CaSO4 from CaCO3, we need to follow these steps:
1. Determine the molar mass of CaCO3:
- The molar mass of Ca (calcium) is 40.08 g/mol.
- The molar mass of C (carbon) is 12.01 g/mol.
- The molar mass of O (oxygen) is 16.00 g/mol.
- So, the molar mass of CaCO3 is (40.08 + 12.01 + (3 * 16.00)) g/mol = 100.09 g/mol.
2. Convert the given mass of CaCO3 from kg to grams:
- 100 kg = (100 * 1000) g = 100000 g.
3. Calculate the number of moles of CaCO3:
- Moles of CaCO3 = Mass of CaCO3 / Molar mass of CaCO3 = 100000 g / 100.09 g/mol.
4. Since the balanced chemical equation for the reaction is:
CaCO3 + H2SO4 → CaSO4 + H2O + CO2
It tells us that the stoichiometric ratio between CaCO3 and H2SO4 is 1:1. This means that one mole of CaCO3 reacts with one mole of H2SO4.
5. Therefore, the number of moles of H2SO4 required will be the same as the number of moles of CaCO3:
- Moles of H2SO4 = Moles of CaCO3 = 100000 g / 100.09 g/mol.
So, the number of moles of H2SO4 required to produce 100 kg of CaSO4 from CaCO3 is equal to the number of moles of CaCO3, which is approximately 999.95 moles.