Sulfuric acid can dissolve aluminum metal according to the following reaction.

Suppose you wanted to dissolve an aluminum block with a mass of 25.7 .

How many grams of H2 gas would be produced by the complete reaction of the aluminum block?

3H2SO4+ 2Al >> 3H2 + Al2(SO4)3

moles H2=3/2 moles Al=3/2 *massAl/atomicmassAl

grams H2=molesH2*2g/mole

To determine the amount of H2 gas produced by the complete reaction of the aluminum block, we need to use stoichiometry and the balanced chemical equation.

The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and aluminum (Al) is:

2 Al + 3 H2SO4 -> Al2(SO4)3 + 3 H2

According to the equation, 2 moles of aluminum react with 3 moles of sulfuric acid to produce 3 moles of hydrogen gas.

To calculate the amount of H2 gas produced, we need to convert the mass of aluminum to moles using its molar mass. The molar mass of aluminum is 26.98 g/mol.

Given that the mass of aluminum is 25.7 g, we can calculate the number of moles of aluminum as follows:

moles of Al = mass of Al / molar mass of Al
moles of Al = 25.7 g / 26.98 g/mol ≈ 0.952 moles

Now, we can use the stoichiometry of the balanced equation to calculate the moles of H2 gas produced:

moles of H2 = moles of Al x (3 moles H2 / 2 moles Al)
moles of H2 = 0.952 moles x (3/2) ≈ 1.43 moles

Finally, we can convert the moles of H2 gas to grams by multiplying it by the molar mass of hydrogen, which is 2.016 g/mol:

mass of H2 = moles of H2 x molar mass of H2
mass of H2 = 1.43 moles x 2.016 g/mol ≈ 2.89 g

Therefore, approximately 2.89 grams of H2 gas would be produced by the complete reaction of the 25.7-gram aluminum block.