Identify the coefficient of Fe₂O₃(s)when the following reaction is balanced,and determine the number of grams of MgO needed to produce 10.0 g of Fe₂O₃. (unbalanced)MgO(s)+ Fe(s)→ Fe₂O₃(s)+ Mg(s) A)coefficient 2,mass 0.312 g B)coefficient 3,mass 0.841 g C)coefficient 4,mass 2.52 g D)coefficient 1,mass 7.57 g

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The balanced chemical equation is MgO(s) + Fe(s) → Fe_2O_3(s) + Mg(s), where the coefficient of Fe_2O_3 is 1. To find the mass of MgO needed to produce 10.0 g of Fe_2O_3, use molar masses and stoichiometry. The molar mass of Fe_2O_3 is approximately 159.69 g/mol, and the molar mass of MgO is about 40.30 g/mol. Since the reaction is 1:1, (10.0 g Fe_2O_3) / (159.69 g/mol) * (40.30 g/mol) = 2.52 g, which seems like a calculation error. Correct calculation: (10.0 g Fe_2O_3) / (159.69 g/mol) * (40.30 g/mol) gives approximately 2.52 g, indicating a mistake in the explanation. The correct approach involves using the stoichiometry of the balanced equation, but the explanation provided does not accurately calculate the mass of MgO needed based on the stoichiometry given. The correct mass calculation should directly relate to the stoichiometry and molar masses involved.

Identify the Coefficient of Fe2O3(s)when the Following Reaction Is Balanced,and

Identify the Coefficient of Fe₂O₃(s)when the Following Reaction Is Balanced,and