2Al+6HClarrow Al_(2)Cl_(6)+3H_(2) Calculate the mass of hydrogen formed when 25 grams of aluminum reacts with excess hydrochloric acid. a 0.419 b 1.80 g C 2.80 g d 0.929

This is a stoichiometry problem. The balanced chemical equation shows that 2 moles of aluminum (Al) react with 6 moles of hydrochloric acid (HCl) to produce 3 moles of hydrogen (H2). Therefore, the molar ratio of Al to H2 is 2:3. <br /><br />First, we need to convert the mass of aluminum to moles. The molar mass of Al is approximately 26.98 g/mol. So, 25 g of Al is approximately 0.926 moles. <br /><br />Since the molar ratio of Al to H2 is 2:3, we can calculate the moles of H2 produced by multiplying the moles of Al by 3/2. This gives us approximately 1.39 moles of H2. <br /><br />Finally, we convert the moles of H2 to grams using its molar mass, which is approximately 2.02 g/mol. This gives us approximately 2.80 g of H2. Therefore, the mass of hydrogen formed when 25 grams of aluminum reacts with excess hydrochloric acid is approximately 2.80 g.