In the reaction Fe^2O^3+3CO->2FE+3CO^2, what is the total number of moles of CO used to produce 112 grams of iron?
Please explain step by step how to do this problem, thanks:)
how many moles Fe in 112g?
each 2 moles of Fe uses 3 moles CO
Generally, "^" are not used in molecular formulas. Better would be
Fe2O3+3CO->2Fe+3CO2
To determine the total number of moles of CO used to produce 112 grams of iron, you'll need to use the molar masses of the substances involved and apply the concept of stoichiometry.
Step 1: Calculate the molar mass of CO.
The molar mass of carbon (C) is 12.01 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol. Since CO has one carbon atom and one oxygen atom, the molar mass of CO is:
Molar mass of CO = (1 * molar mass of C) + (1 * molar mass of O)
= (1 * 12.01 g/mol) + (1 * 16.00 g/mol)
= 28.01 g/mol
Step 2: Convert the given mass of iron (112 grams) to moles.
To convert the mass of a substance to moles, divide the mass by its molar mass. The molar mass of iron (Fe) is 55.85 g/mol.
Number of moles of Fe = 112 g / (55.85 g/mol) ≈ 2.003 moles
Step 3: Apply the stoichiometry of the balanced chemical equation.
From the balanced chemical equation Fe2O3 + 3CO -> 2Fe + 3CO2, you can see that 1 mole of Fe2O3 reacts with 3 moles of CO to produce 2 moles of Fe.
So, the number of moles of CO used to produce 2.003 moles of Fe is:
Number of moles of CO = (3 moles of CO / 1 mole of Fe2O3) * 2.003 moles of Fe
= 6.009 moles
Therefore, the total number of moles of CO used to produce 112 grams of iron is approximately 6.009 moles of CO.