QuestionFebruary 10, 2026

3. How many grams of Fe_(2)(SO_(4))_(3) will be produced from 4.25 moles of Fe? 2Fe+3H_(2)SO_(4)arrow 1Fe_(2)(SO_(4))_(3)+3H_(2)

3. How many grams of Fe_(2)(SO_(4))_(3) will be produced from 4.25 moles of Fe? 2Fe+3H_(2)SO_(4)arrow 1Fe_(2)(SO_(4))_(3)+3H_(2)
3. How many grams of Fe_(2)(SO_(4))_(3) will be produced from 4.25 moles of Fe? 2Fe+3H_(2)SO_(4)arrow 1Fe_(2)(SO_(4))_(3)+3H_(2)

Solution
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Answer

849.84\ \text{g} Explanation 1. Determine mole ratio From 2Fe \rightarrow 1Fe_{2}(SO_{4})_{3}, mole ratio Fe : Fe_{2}(SO_{4})_{3} is 2:1. 4.25 mol Fe × \frac{1}{2} = 2.125 mol Fe_{2}(SO_{4})_{3}. 2. Calculate molar mass of Fe_{2}(SO_{4})_{3} M = 2(55.85) + 3[32.06 + 4(16.00)] = 111.70 + 3(96.06) = 111.70 + 288.18 = 399.88\ \text{g/mol}. 3. Calculate mass produced m = n \times M = 2.125 \times 399.88 = 849.835\ \text{g} \approx 849.84\ \text{g}.

Explanation

1. Determine mole ratio <br /> From $2Fe \rightarrow 1Fe_{2}(SO_{4})_{3}$, mole ratio Fe : $Fe_{2}(SO_{4})_{3}$ is $2:1$. <br />$4.25$ mol Fe × $\frac{1}{2} = 2.125$ mol $Fe_{2}(SO_{4})_{3}$. <br /><br />2. Calculate molar mass of $Fe_{2}(SO_{4})_{3}$ <br /> $M = 2(55.85) + 3[32.06 + 4(16.00)] = 111.70 + 3(96.06) = 111.70 + 288.18 = 399.88\ \text{g/mol}$. <br /><br />3. Calculate mass produced <br /> $m = n \times M = 2.125 \times 399.88 = 849.835\ \text{g} \approx 849.84\ \text{g}$.
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