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 H _{2}SO_{4}(aq) + 22 H_{2}O(l) → 2 KAl(SO_{4})_{2}•12H_{2}O(s) + 3 H_{2}(g)**

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

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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