During a “Synthesis of Alum” experiment, a student uses 0.495 g of aluminum foil and dissolves it with 25.3 mL of 1.4 M KOH. After cooling the mixture, the student adds 11.9 mL of 9.0 M H2SO4. a. Calculate the formula weight (or molar mass) of alum. Don’t forget to include the 12 waters of hydration. b. Use 2Al(s) + 2KOH(aq) + 4H2SO4(aq) + 22H2O(l) → 3H2(g) + 2KAl(SO4)2 ⋅ 12H2O(s) to calculate the theoretical yield based on each of the reactants. c. If the student isolated 5.042 g of alum, calculate the percent yield.
During a “Synthesis of Alum” experiment, a student uses 0.495 g of aluminum foil and dissolves it with 25.3 mL of 1.4 M KOH. After cooling the mixture, the student adds 11.9 mL of 9.0 M H2SO4. a. Calculate the formula weight (or molar mass) of alum. Don’t forget to include the 12 waters of hydration. b. Use 2Al(s) + 2KOH(aq) + 4H2SO4(aq) + 22H2O(l) → 3H2(g) + 2KAl(SO4)2 ⋅ 12H2O(s) to calculate the theoretical yield based on each of the reactants. c. If the student isolated 5.042 g of alum, calculate the percent yield.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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During a “Synthesis of Alum” experiment, a student uses 0.495 g of aluminum foil and dissolves it with 25.3 mL of 1.4 M KOH. After cooling the mixture, the student adds 11.9 mL of 9.0 M H2SO4.
a. Calculate the formula weight (or molar mass) of alum. Don’t forget to include the 12 waters of hydration.
b. Use 2Al(s) + 2KOH(aq) + 4H2SO4(aq) + 22H2O(l) → 3H2(g) + 2KAl(SO4)2 ⋅ 12H2O(s) to calculate the theoretical yield based on each of the reactants.
c. If the student isolated 5.042 g of alum, calculate the percent yield.
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