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Answer to Question #66274 in General Chemistry for Tony
Question #66274
Calculate the number of grams (theoretical yield) of the final iron complex that can be produced from 10.00 g?
Calculate the number of grams (theoretical yield) of the final iron complex that can be produced from 10.00 g of ferrous ammonium sulfate hexahydrate. Show all your work. (hints: the mole relationship of reactant to product can be found in the equation for the overall synthesis. Also when determining the molar masses, you must include the waters of hydration. For instance if the are two waters of hydration add 36g/mole.)
Calculate the number of grams (theoretical yield) of the final iron complex that can be produced from 10.00 g of ferrous ammonium sulfate hexahydrate. Show all your work. (hints: the mole relationship of reactant to product can be found in the equation for the overall synthesis. Also when determining the molar masses, you must include the waters of hydration. For instance if the are two waters of hydration add 36g/mole.)
Expert's answer
(NH₄)₂SO₄*FeSO₄*6H₂O=>[Fe(H₂O)₆]SO₄+(NH₄)₂SO₄
M(NH₄)₂SO₄*FeSO₄*6H₂O)=392g/Mol
M([Fe(H₂O)₆]SO₄)=260g/Mol
m([Fe(H₂O)₆SO₄)=260g/Mol*10g/392g/Mol=6.633g
M(NH₄)₂SO₄*FeSO₄*6H₂O)=392g/Mol
M([Fe(H₂O)₆]SO₄)=260g/Mol
m([Fe(H₂O)₆SO₄)=260g/Mol*10g/392g/Mol=6.633g
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