2Fe2O3 + 6C + 3O2 -> 4Fe + 6Co2
What mass of Fe2O3 present is needed to produce 15 of iron?
what mass of CO2 is released when 15g of iron is produced?
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To find the mass of Fe2O3 needed to produce 15g of iron, we need to use the balanced chemical equation and the molar masses of the compounds involved.
First, let's calculate the molar mass of Fe2O3 (iron(III) oxide). The molar mass of Fe is 55.85 g/mol, and the molar mass of O is 16.00 g/mol. Since there are two iron atoms and three oxygen atoms in Fe2O3, the molar mass can be calculated as follows:
Fe2O3: (2 * 55.85 g/mol) + (3 * 16.00 g/mol) = 159.70 g/mol
Next, we need to determine the stoichiometric coefficient relating Fe2O3 and Fe in the balanced chemical equation. From the equation given, we see that 2 moles of Fe2O3 produce 4 moles of Fe.
Now, we can set up a proportion to find the mass of Fe2O3 needed:
(2 moles Fe2O3 / 4 moles Fe) = (x g Fe2O3 / 15 g Fe)
Solving for x, we can cross-multiply and divide:
x g Fe2O3 = (2 moles Fe2O3 / 4 moles Fe) * 15 g Fe
x g Fe2O3 = (2/4) * 15 g Fe
x g Fe2O3 = 7.5 g Fe2O3
Therefore, you will need 7.5 grams of Fe2O3 to produce 15g of iron.
To find the mass of CO2 released when 15g of iron is produced, we can use the same approach.
From the balanced equation, we see that 4 moles of Fe produce 6 moles of CO2.
First, calculate the molar mass of CO2 (carbon dioxide). The molar mass of C is 12.01 g/mol, and the molar mass of O is 16.00 g/mol.
CO2: (1 * 12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol
Now, we can set up a proportion:
(4 moles Fe / 6 moles CO2) = (15 g Fe / x g CO2)
Solving for x:
x g CO2 = (4 moles Fe / 6 moles CO2) * 15 g Fe
x g CO2 = (4/6) * 15 g Fe
x g CO2 = 10 g CO2
Therefore, 10 grams of CO2 will be released when 15g of iron is produced.