12FeCl2(s) + 3O2(g) → 8FeCl3(s) + 2Fe2O3(s) 1. Determine the theoretical and actual yield of Fe2O3 if 153.00 g of FeCl 2 and 12.15 g of O 2 react, and the percent yield of Fe2O3 is 61.55%. (Molar masses are FeCl2 = 126.75 g/mol, FeCl3 = 162.20 g/mol, Fe2O3 = 159.69 g/mol)
12FeCl2(s) + 3O2(g) → 8FeCl3(s) + 2Fe2O3(s) 1. Determine the theoretical and actual yield of Fe2O3 if 153.00 g of FeCl 2 and 12.15 g of O 2 react, and the percent yield of Fe2O3 is 61.55%. (Molar masses are FeCl2 = 126.75 g/mol, FeCl3 = 162.20 g/mol, Fe2O3 = 159.69 g/mol)
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 157QRT
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12FeCl2(s) + 3O2(g) → 8FeCl3(s) + 2Fe2O3(s)
1. Determine the theoretical and actual yield of Fe2O3 if 153.00 g of FeCl 2 and 12.15 g of O 2 react, and the percent yield
of Fe2O3 is 61.55%. (Molar masses are FeCl2 = 126.75 g/mol, FeCl3 = 162.20 g/mol, Fe2O3 = 159.69 g/mol)
of Fe2O3 is 61.55%. (Molar masses are FeCl2 = 126.75 g/mol, FeCl3 = 162.20 g/mol, Fe2O3 = 159.69 g/mol)
2. Consider at 4.5 M stock solution of glucose (C6H12O6, 180.156 g/mol).
(a) How many grams of glucose are needed to produced 500. mL of the stock solution.
(b) If 15.0 mL of the stock solution was diluted to a total volume of 250 mL, the concentration of the resulting solution is?
(a) How many grams of glucose are needed to produced 500. mL of the stock solution.
(b) If 15.0 mL of the stock solution was diluted to a total volume of 250 mL, the concentration of the resulting solution is?
3. A solution of HClO 4 , a strong acid can be neutralized by adding solid Cu(OH)2 .
(a) Write the net ionic equation describing the reaction between HClO4 , and Cu(OH)2
(b) How many grams of Cu(OH)2 are needed to neutralize 25.0 mL of 0.500 M HClO 4 ,?
(a) Write the net ionic equation describing the reaction between HClO4 , and Cu(OH)2
(b) How many grams of Cu(OH)2 are needed to neutralize 25.0 mL of 0.500 M HClO 4 ,?
4.When 75.0 mL of 0.455 M Al(NO 3 )2 and 110 mL of 0.312 M Na2 CO3 are mixed a precipitate forms.
(a) Write the net ionic equation describing the formation of the precipitate
(b) What is the (theoretical) mass of the precipitate that forms?
(a) Write the net ionic equation describing the formation of the precipitate
(b) What is the (theoretical) mass of the precipitate that forms?
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