# Problem: Sulfuric acid dissolves aluminum metal according to the following reaction: 2 Al(s) + 3H2SO4 (aq) → Al2(SO4)3 (aq) + 3H2 (g)Suppose you wanted to dissolve an aluminum block with a mass of 14.3 g. What minimum mass of H2SO4 would you need? Express your answer in grams.What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams.

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###### FREE Expert Solution
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###### Problem Details

Sulfuric acid dissolves aluminum metal according to the following reaction:

2 Al(s) + 3H2SO4 (aq) → Al2(SO4)3 (aq) + 3H2 (g)

Suppose you wanted to dissolve an aluminum block with a mass of 14.3 g.

What minimum mass of H2SO4 would you need? Express your answer in grams.

What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems .

What is the difficulty of this problem?

Our tutors rated the difficulty of Sulfuric acid dissolves aluminum metal according to the foll... as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 6 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Perry's class at NSU.