Question

Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 15.4 gg .
What minimum mass of H2SO4 would you need?

What mass of H2 gas would be produced by the complete reaction of the aluminum block?

Answer 1

Answer:

83.9g of sulfuric acid is the minimum mass you would need

1.73g of hydrogen would be produced

Explanation:

Based on the reaction:

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

2 moles of solid aluminium react with 3 moles of sulfuric acid. Also, two moles of Al produce 3 moles of hydrogen gas.

15.4g of Al are:

15.4g Al × (1mol / 26.98g) = 0.571 moles of Al.

Moles of sulfuric acid:

0.571 moles Al × (3 mol H₂SO₄ / 2 mol Al) = 0.8565 moles H₂SO₄

In grams:

0.8565 moles H₂SO₄ × (98g / 1mol) = 83.9g of sulfuric acid is the minimum mass you would need

In the same way, moles of hydrogen produced are:

0.571 moles Al × (3 mol H₂ / 2 mol Al) = 0.8565 moles H₂

In grams:

0.8565 moles H₂ × (2.015g / 1mol) = 1.73g of hydrogen would be produced