Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 49.1 mL of hydrogen gas over water at 27°C and 751 mmHgHow many grams of aluminum reacted?I keep getting 0.035 g Al and it says it's wrongPlease help!
Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 49.1 mL of hydrogen gas over water at 27°C and 751 mmHgHow many grams of aluminum reacted? Balanced Equation 2Al + 6 HCl → 2 AlCl3 + 3 H2 (g) According to the balanced equation, 2 moles of Al react with 6 moles of HCl to produce 2 moles of AlCl3 and 3 moles of H2 gasAt Standard temperature and pressure, 1 mole of H2 has a volume of 22.4 litersSo, you need to convert the volume at 27°C and 751 mmHg, to the volume at STPStandard temperature 0° C 273°K Standard pressure 760 mm Hg Set up a proportion: (P1 V1) / T1 (760 V stp) / 273 P1 751 V1 49.1 ml 0.0491 L T1 27 + 273 300°K (751 0.0491) / 300 (760 V stp) / 273 Vstp 0.04415 L At Standard temperature and pressure, 1 mole of H2 has a volume of 22.4 litersset up a proportion 1 mole / 22.4L x / 0.04415 x 0.001971 moles of H2 gas According to the balanced equation, (2 moles of Al) react with 6 moles of HCl to produce 2 moles of AlCl3 and (3 moles of H2 gas set up proportion 2 moles Al / 3 moles H2 x /0.001971 moles of H2 x (? 0.001971) moles of Al Mass of Al moles of Al (molar mass) Mass of Al (? 0.001971) 27 0.03548 g of Al Round as your instructor desires
