QuestionMay 6, 2025

Consider the following reaction: 3O_(2)+4Fearrow 2Fe_(2)O_(3) How many moles of Fe are consumed when 29.3 grams of Fe_(2)O_(3) are produced in the reaction above? Round to 3 significant figures.

Consider the following reaction: 3O_(2)+4Fearrow 2Fe_(2)O_(3) How many moles of Fe are consumed when 29.3 grams of Fe_(2)O_(3) are produced in the reaction above? Round to 3 significant figures.
Consider the following reaction: 3O_(2)+4Fearrow 2Fe_(2)O_(3) How many moles of Fe are consumed when 29.3 grams of Fe_(2)O_(3) are produced in the reaction above? Round to 3 significant figures.

Solution
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Answer

0.367 moles of Fe are consumed. Explanation 1. Calculate moles of Fe_{2}O_{3} produced Molar mass of Fe_{2}O_{3} is 2(55.85) + 3(16.00) = 159.7 \, g/mol. Moles of Fe_{2}O_{3} = \frac{29.3 \, g}{159.7 \, g/mol}. 2. Use stoichiometry to find moles of Fe consumed From the balanced equation, 2 \, mol \, Fe_{2}O_{3} requires 4 \, mol \, Fe. Therefore, moles of Fe = moles of Fe_{2}O_{3} \times \frac{4}{2}.

Explanation

1. Calculate moles of $Fe_{2}O_{3}$ produced<br /> Molar mass of $Fe_{2}O_{3}$ is $2(55.85) + 3(16.00) = 159.7 \, g/mol$. Moles of $Fe_{2}O_{3}$ = $\frac{29.3 \, g}{159.7 \, g/mol}$.<br /><br />2. Use stoichiometry to find moles of Fe consumed<br /> From the balanced equation, $2 \, mol \, Fe_{2}O_{3}$ requires $4 \, mol \, Fe$. Therefore, moles of Fe = moles of $Fe_{2}O_{3} \times \frac{4}{2}$.
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