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The increased weight of 0.606 - 0.424 = 0.182 (g) must be due to oxygen. Since Fe has atomic weight of 55.845, and Oxygen 16.00. Hence in 0.606g reddish brown oxide, 0.424g iron is 0.424/55.845 Mol = 0.00759 Mol, and 0.182g oxygen is 0.182/16.00 Mol = 0.01138 Mol. Since 0.01138/0.00759 = 1.4982 ≈ 1.5, the emperical must be Fe2O3.
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The increased weight of 0.606 - 0.424 = 0.182 (g) must be due to oxygen. Since Fe has atomic weight of 55.845, and Oxygen 16.00. Hence in 0.606g reddish brown oxide, 0.424g iron is 0.424/55.845 Mol = 0.00759 Mol, and 0.182g oxygen is 0.182/16.00 Mol = 0.01138 Mol. Since 0.01138/0.00759 = 1.4982 ≈ 1.5, the emperical must be Fe2O3.
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