Calculate the number of grams of Fe formed when 0.350 kg of Fe2O3 reacts.
m = g
To calculate the number of grams of Fe formed, we need to use stoichiometry and the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between Fe2O3 and Fe is:
Fe2O3 + 3Fe --> 2Fe2O3
From the balanced equation, we can see that 1 mole of Fe2O3 reacts with 3 moles of Fe. To find the number of moles of Fe2O3, we can use the given mass and the molar mass of Fe2O3.
First, we need to convert the given mass of Fe2O3 from kilograms to grams:
0.350 kg = 350 grams
Next, we need to find the molar mass of Fe2O3. The molar mass of Fe is 55.845 g/mol and the molar mass of O is 16.00 g/mol. Since there are two moles of Fe atoms and three moles of O atoms in one mole of Fe2O3, we can calculate the molar mass:
Molar mass of Fe2O3 = (2 * molar mass of Fe) + (3 * molar mass of O)
= (2 * 55.845 g/mol) + (3 * 16.00 g/mol)
= 159.69 g/mol
Next, we can calculate the number of moles of Fe2O3:
moles of Fe2O3 = mass of Fe2O3 / molar mass of Fe2O3
= 350 grams / 159.69 g/mol
= 2.19 moles
According to the balanced chemical equation, for every 1 mole of Fe2O3, 3 moles of Fe are formed. Therefore, we can use this ratio to calculate the number of moles of Fe formed:
moles of Fe = moles of Fe2O3 * (3 moles of Fe / 1 mole of Fe2O3)
= 2.19 moles * (3 moles of Fe / 1 mole of Fe2O3)
= 6.57 moles
Finally, we can convert the moles of Fe to grams using the molar mass of Fe:
mass of Fe = moles of Fe * molar mass of Fe
= 6.57 moles * 55.845 g/mol
= 367.15 grams
Therefore, when 0.350 kg of Fe2O3 reacts, approximately 367.15 grams of Fe are formed.