QuestionJune 2, 2025

If you cannot read this diagram, use the diagram you made. Question 1: How many grams of solid iron will be produced from 55.5 grams of iron (III) oxide? Fe_(2)O_(3)(s)+3CO(g)Longrightarrow 2Fe(s)+3CO_(2)(g)

If you cannot read this diagram, use the diagram you made. Question 1: How many grams of solid iron will be produced from 55.5 grams of iron (III) oxide? Fe_(2)O_(3)(s)+3CO(g)Longrightarrow 2Fe(s)+3CO_(2)(g)
If you cannot read this diagram, use the diagram you made.
Question 1: How many grams of solid iron will be produced from 55.5 grams of iron (III) oxide?
Fe_(2)O_(3)(s)+3CO(g)Longrightarrow 2Fe(s)+3CO_(2)(g)

Solution
4.3(286 votes)

Answer

38.8 grams of solid iron will be produced. Explanation 1. Calculate moles of Fe_2O_3 Molar mass of Fe_2O_3 is 2(55.85) + 3(16.00) = 159.7 \, g/mol. Moles of Fe_2O_3 = \frac{55.5 \, g}{159.7 \, g/mol}. 2. Use stoichiometry to find moles of Fe From the balanced equation, 1 mole of Fe_2O_3 produces 2 moles of Fe. Multiply moles of Fe_2O_3 by 2. 3. Convert moles of Fe to grams Molar mass of Fe is 55.85 \, g/mol. Grams of Fe = moles of Fe \times 55.85 \, g/mol.

Explanation

1. Calculate moles of $Fe_2O_3$<br /> Molar mass of $Fe_2O_3$ is $2(55.85) + 3(16.00) = 159.7 \, g/mol$. Moles of $Fe_2O_3 = \frac{55.5 \, g}{159.7 \, g/mol}$.<br /><br />2. Use stoichiometry to find moles of Fe<br /> From the balanced equation, 1 mole of $Fe_2O_3$ produces 2 moles of Fe. Multiply moles of $Fe_2O_3$ by 2.<br /><br />3. Convert moles of Fe to grams<br /> Molar mass of Fe is $55.85 \, g/mol$. Grams of Fe = moles of Fe $\times 55.85 \, g/mol$.
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