The balanced chemical equation for the reaction between aluminum (Al) and sulfuric acid (H2SO4) is:
2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)
From the balanced equation, we can see that 2 moles of aluminum react with 3 moles of sulfuric acid to produce 3 moles of hydrogen gas.
Given that you have 25.0 moles of aluminum, we can use the stoichiometry of the balanced equation to determine the corresponding amount of sulfuric acid required.
Using a ratio of 2 moles of aluminum to 3 moles of sulfuric acid, we can set up the following proportion:
(2 moles Al / 3 moles H2SO4) = (25.0 moles Al / x moles H2SO4)
Cross-multiplying and solving for x, we get:
x = (3 moles H2SO4 * 25.0 moles Al) / 2 moles Al
x = 37.5 moles H2SO4
Therefore, 37.5 moles of sulfuric acid are needed to completely react with 25.0 moles of aluminum.