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Problem: When 4.50 g of Fe2O3 is reduced with excess H2 in a furnace, 2.60 g of metallic iron is recovered. What is the percent yield? This is the equation representing the reaction. Fe2O3 has a molar mass of 159.7 g x mol-1 Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g) a) 82.6% b) 70.0% c) 57.8% d) 31.5%

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When 4.50 g of Fe2O3 is reduced with excess H2 in a furnace, 2.60 g of metallic iron is recovered. What is the percent yield? This is the equation representing the reaction. Fe2O3 has a molar mass of 159.7 g x mol-1

Fe2O(s) + 3 H(g) → 2 Fe (s) + 3 H2O (g)

a) 82.6%

b) 70.0%

c) 57.8%

d) 31.5%

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