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If Fe2O3 + c → co + Fernrn4.89 moles of c are reacted with 2.390 moles of Fe2O3, how many grams of co will be produced if the reaction proceeds with a 79% yield?
Accepted Answer
The balanced chemical equation is:
Fe2O3 + 3C → 3CO + 2Fe
From the stoichiometry of the balanced chemical equation, the mole ratio between C and CO is 3:3 or 1:1.
Therefore, 4.89 moles of C will react with 4.89 moles of CO.
The molar mass of CO is 28.01 g/mol.
Therefore, the mass of 4.89 moles of CO is:
4.89 moles CO × 28.01 g/mol CO = 136.6 g CO
However, the reaction only proceeds with a 79% yield. Therefore, the actual mass of CO produced will be:
136.6 g CO × 0.79 = 108.0 g CO (rounded to three significant figures)
Therefore, 108.0 grams of CO will be produced if the reaction proceeds with a 79% yield.
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