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 Al(s) + 2 KOH(aq) + 4 H2SO4(aq) + 22 H2O(l) → 2 KAl(SO4)2•12H2O(s) + 3 H2(g)What is the mass of Alum theoretically possible? (Hint – Use the molar mass of the alum calculated in question #1.)

Question
Asked Sep 30, 2019

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 Al(s) + 2 KOH(aq) + 4 H2SO4(aq) + 22 H2O(l) → 2 KAl(SO4)2•12H2O(s) + 3 H2(g)

What is the mass of Alum theoretically possible? (Hint – Use the molar mass of the alum calculated in question #1.)

check_circleExpert Solution
Step 1

Given:

Mass of Al= 2.583 grams

Chemical equation:

2 Al(s) + 2 KOH(aq) + 4 H2SO4(aq) + 22 H2O(l) → 2 KAl (SO4)2•12H2O(s) + 3 H2(g)

From the balanced chemical equation,

  2mol × 26.981g/mol= 53.962g of Al ca...

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