Sulfuric acid can dissolve aluminum metal according to the following reaction.
2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 23.7 g .
Sulfuric acid can dissolve aluminum metal according to the following reaction.
2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 23.7 g .
and the question is?
To determine the amount of sulfuric acid needed to dissolve the aluminum block, you'll first need to calculate the molar mass of aluminum (Al) and sulfuric acid (H2SO4).
The molar mass of aluminum (Al) is 26.98 g/mol.
The molar mass of sulfuric acid (H2SO4) can be calculated as follows:
- The molar mass of hydrogen (H) is 1.01 g/mol.
- The molar mass of sulfur (S) is 32.07 g/mol.
- The molar mass of oxygen (O) is 16.00 g/mol.
Thus, the molar mass of sulfuric acid (H2SO4) is:
(2 * 1.01 g/mol) + (32.07 g/mol) + (4 * 16.00 g/mol) = 98.09 g/mol.
Now, using the balanced chemical equation, we can determine the molar ratio between aluminum and sulfuric acid:
2 moles of Al reacts with 3 moles of H2SO4.
To find the moles of aluminum (Al), divide the given mass of aluminum (23.7 g) by its molar mass (26.98 g/mol):
Moles of Al = 23.7 g / 26.98 g/mol = 0.88 mol.
Using the molar ratio, you can determine the moles of sulfuric acid (H2SO4) needed to fully react with the aluminum:
Moles of H2SO4 = (0.88 mol Al) * (3 mol H2SO4 / 2 mol Al) = 1.32 mol.
Finally, to find the mass of sulfuric acid needed, multiply the moles of H2SO4 by its molar mass:
Mass of H2SO4 = (1.32 mol) * (98.09 g/mol) = 129.32 g.
Therefore, to dissolve the aluminum block with a mass of 23.7 g, you will need approximately 129.32 grams of sulfuric acid.