QuestionJune 8, 2025

2Fe_(2)O_(3)(s)+3C(s)arrow 4Fe(s)+3CO_(2)(g) Calculate the mass of iron produced from the complete reaction of 64.0 grams of iron (III)oxide. 89.5 g Fe 22.48 Fe 11.2 g Fe 44.88 Fe 107 g Fe

2Fe_(2)O_(3)(s)+3C(s)arrow 4Fe(s)+3CO_(2)(g) Calculate the mass of iron produced from the complete reaction of 64.0 grams of iron (III)oxide. 89.5 g Fe 22.48 Fe 11.2 g Fe 44.88 Fe 107 g Fe
2Fe_(2)O_(3)(s)+3C(s)arrow 4Fe(s)+3CO_(2)(g) Calculate the mass of iron produced from the complete reaction of 64.0 grams of iron (III)oxide. 89.5 g Fe 22.48 Fe 11.2 g Fe 44.88 Fe 107 g Fe

Solution
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Answer

44.72 g Fe Explanation 1. Calculate Molar Mass of Fe_2O_3 Molar mass of Fe_2O_3 = 2 \times 55.85 + 3 \times 16.00 = 159.7 g/mol. 2. Determine Moles of Fe_2O_3 Moles of Fe_2O_3 = \frac{64.0 \text{ g}}{159.7 \text{ g/mol}} = 0.4005 mol. 3. Use Stoichiometry to Find Moles of Fe From the balanced equation, 2 \text{ mol } Fe_2O_3 \rightarrow 4 \text{ mol } Fe. Thus, 0.4005 \text{ mol } Fe_2O_3 \rightarrow 0.4005 \times 2 = 0.801 \text{ mol } Fe. 4. Calculate Mass of Iron Produced Mass of Fe = 0.801 \text{ mol} \times 55.85 \text{ g/mol} = 44.72 \text{ g}.

Explanation

1. Calculate Molar Mass of $Fe_2O_3$<br /> Molar mass of $Fe_2O_3 = 2 \times 55.85 + 3 \times 16.00 = 159.7$ g/mol.<br /><br />2. Determine Moles of $Fe_2O_3$<br /> Moles of $Fe_2O_3 = \frac{64.0 \text{ g}}{159.7 \text{ g/mol}} = 0.4005$ mol.<br /><br />3. Use Stoichiometry to Find Moles of Fe<br /> From the balanced equation, $2 \text{ mol } Fe_2O_3 \rightarrow 4 \text{ mol } Fe$. Thus, $0.4005 \text{ mol } Fe_2O_3 \rightarrow 0.4005 \times 2 = 0.801 \text{ mol } Fe$.<br /><br />4. Calculate Mass of Iron Produced<br /> Mass of Fe = $0.801 \text{ mol} \times 55.85 \text{ g/mol} = 44.72 \text{ g}$.
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