Sulfuric acid dissolves 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 14.9g .What minimum mass of H2SO4 would you need? What mass of H2 gas would be produced by the complete reaction of the aluminum block?

Go back and look at the NaCl/Cl2/H2 problem you posted earlier. Those steps are the same for solving this problem. If you need help show where your trouble is and we an help you through.

To determine the minimum mass of H2SO4 needed and the mass of H2 gas produced, we need to use stoichiometry, which relates the moles of reactants and products in a chemical equation.

First, let's calculate the moles of aluminum (Al) in the aluminum block. We can do this by dividing the mass of Al by its molar mass, which is 26.98 g/mol.

Moles of Al = Mass of Al / Molar mass of Al
Moles of Al = 14.9 g / 26.98 g/mol

Next, we need to use the mole ratio between Al and H2SO4 from the balanced chemical equation. From the equation, we can see that the ratio between Al and H2SO4 is 2:3.

Moles of H2SO4 = (Moles of Al * 3) / 2

Now, to find the mass of H2SO4 needed, we multiply the moles of H2SO4 by its molar mass, which is 98.09 g/mol.

Mass of H2SO4 = Moles of H2SO4 * Molar mass of H2SO4

Finally, to determine the mass of H2 gas produced, we need to use the mole ratio between Al and H2 from the balanced chemical equation. From the equation, we can see that the ratio between Al and H2 is 2:3.

Moles of H2 = (Moles of Al * 3) / 2

To find the mass of H2 gas, multiply the moles of H2 by its molar mass, which is 2.02 g/mol.

Mass of H2 gas = Moles of H2 * Molar mass of H2

By following these steps, we can calculate the minimum mass of H2SO4 needed and the mass of H2 gas produced in the reaction.