2. A student used a piece of aluminum that had a mass of 2.583 grams, and treated according to the same procedure you used in this experiment. 2 A1(s)+2 KOH(aq) + 4 H2SO4(aq) +22 H200) 2 KAI(SO4)2 12H20(s) +3 H2(g) How many moles of Al did the student use in this experiment? a. How many moles of the Alum, KAI(SO42 * 12 H20, Use the coefficients from the balanced chemical equation.) b. can be produced theoretically? (Hint- What is the mass of Alum theoretically possible? (Hint - Use the molar mass of the alum calculated in question #1.) c. d. If the student's crystals had a mass of 32.105 g, what is the percent yield?

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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2. A student used a piece of aluminum that had a mass of 2.583 grams, and treated according to the
same procedure you used in this experiment.
2 A1(s)+2 KOH(aq) + 4 H2SO4(aq) +22 H200) 2 KAI(SO4)2 12H20(s) +3 H2(g)
How many moles of Al did the student use in this experiment?
a.
How many moles of the Alum, KAI(SO42 * 12 H20,
Use the coefficients from the balanced chemical equation.)
b.
can be produced theoretically? (Hint-
What is the mass of Alum theoretically possible? (Hint - Use the molar mass of the alum
calculated in question #1.)
c.
d. If the student's crystals had a mass of 32.105 g, what is the percent yield?
Transcribed Image Text:2. A student used a piece of aluminum that had a mass of 2.583 grams, and treated according to the same procedure you used in this experiment. 2 A1(s)+2 KOH(aq) + 4 H2SO4(aq) +22 H200) 2 KAI(SO4)2 12H20(s) +3 H2(g) How many moles of Al did the student use in this experiment? a. How many moles of the Alum, KAI(SO42 * 12 H20, Use the coefficients from the balanced chemical equation.) b. can be produced theoretically? (Hint- What is the mass of Alum theoretically possible? (Hint - Use the molar mass of the alum calculated in question #1.) c. d. If the student's crystals had a mass of 32.105 g, what is the percent yield?
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