calculate the number of moles of Al2O3 that are produced when .60 mol of Fe is produced in the following reaction. 2Al(s) +3FeO = 3Fe(s) + Al2O3(s)
To calculate the number of moles of Al2O3 produced, we need to use the balanced chemical equation and the stoichiometry of the reaction.
The stoichiometric ratio tells us the molar relationship between the reactants and products in a chemical reaction. From the balanced equation:
2Al(s) + 3FeO = 3Fe(s) + Al2O3(s)
We can see that 2 moles of Al (Aluminum) react with 3 moles of FeO (Iron(II) oxide) to produce 3 moles of Fe (Iron) and 1 mole of Al2O3 (Aluminum oxide).
Now, we are given that 0.60 mol of Fe is produced. Since the stoichiometric ratio is 2:3 for Al:Fe, we can calculate the moles of Al2O3 using a simple proportion:
(0.60 mol Fe / 3 mol Fe) x 1 mol Al2O3 = 0.20 mol Al2O3
Therefore, when 0.60 mol of Fe is produced, 0.20 mol of Al2O3 is also produced.
To determine the number of moles of Al2O3 produced, we need to use the stoichiometry of the balanced equation.
From the balanced equation:
2 moles of Al reacts with 3 moles of FeO to produce 3 moles of Fe and 1 mole of Al2O3.
We know that 0.60 moles of Fe is produced. According to the stoichiometry, 3 moles of Fe are produced for every 1 mole of Al2O3 produced.
Therefore, the number of moles of Al2O3 produced can be calculated as follows:
0.60 mol Fe * (1 mol Al2O3 / 3 mol Fe) = 0.20 mol Al2O3
So, 0.20 moles of Al2O3 are produced when 0.60 moles of Fe is produced in the given reaction.
2Al(s) +3FeO = 3Fe(s) + Al2O3(s)
The coefficients tell you.
0.6 mol Fe x (1 mol Al2O3/3 mol Fe) = 0.6 x 1/3 = ?