Question

2. Write a balanced chemical reaction for the production of hydrogen gas from aluminum metal and hydrochloric acid. a. What is the expected yield of hydrogen gas (in moles) if 0.06 g of aluminum metal were reacted with HCl in the experiment instead of magnesium? Assume that HCl is in excess. b. What is the expected yield of hydrogen gas (in mL) if the 0.06 g of aluminum metal were reacted with HCl in the experiment instead of magnesium?

Answer 1

Solution - Balance chemical Reaction 2Al(s) + 6HC1 - 2AlCl3 + 3H2 (9) mass of Al = 0.069 (molar mass of A1 = 27g/mol) so mole of A1 = 0.069 -0.00222 mole. 27 g/mol According to balance Reaction Hal in excess? So limiting Reactent is AL Then ? mol Al Produce 3 mol H₂ 1 mol All Produce 3 mol H₂ 0.00222 mol Al Produce 3x0*00222 mole H₂ Thoertical yield of Hp = 0.0033 3 mole Ando b) Thoeotical vield of Hy = 0.00 333moke (from purt a) molar mass of H₂ = 2.02 g/mole. Do. mass of Hy guys 000333 mole 2'02 g 7 Density = mass ) volume mass more = 0.00672669 . Density of H₂ gus = 0.0000 8g glime, Thoertical yield of Hz in me = 75.57 ml "Ang ( volume Density) (v= 0.0067266g . 0.0000899/mo =75.57mi