Calculate how much charcoal(carbon) is needed to reduce 40kg of Fe2O3
2Fe2O3 + 3C ==> 3CO2 + 4Fe
mols Fe2O3 = grams/molar mass
Using the coefficients in the balanced equation, convert mols Fe2O3 to mols C.
If you want C in grams, then g C = mols C x atomic mass C.
To calculate how much charcoal (carbon) is needed to reduce 40 kg of Fe2O3, we need to use the balanced chemical equation for the reaction between carbon and Fe2O3.
The balanced chemical equation for this reaction is:
Fe2O3 + 3C -> 2Fe + 3CO
From the equation, we can see that for every 1 mole of Fe2O3, we need 3 moles of carbon (C) to completely react.
1 mole of Fe2O3 is equal to its molar mass, which is:
2(55.845 g/mol) + 3(16.00 g/mol) = 159.70 g/mol
To find the number of moles of Fe2O3 in 40 kg, we need to convert the mass to grams first:
40 kg * 1000 g/kg = 40000 g
Then, we can calculate the number of moles of Fe2O3:
40000 g / 159.70 g/mol = 250.39 mol
Since the stoichiometric ratio between carbon and Fe2O3 is 3:1, we need 3 times the number of moles of carbon (C):
3 * 250.39 mol = 751.18 mol
Finally, to convert the number of moles of carbon (C) to mass, we multiply by its molar mass, which is 12.01 g/mol:
751.18 mol * 12.01 g/mol = 9018.48 g
Therefore, approximately 9018.48 grams (or 9.01848 kg) of charcoal (carbon) is needed to reduce 40 kg of Fe2O3.