Question

Lean 1 Learning Objective: 7J Distinguish between actual and theoretical yield to calculate percent yield Question A0.156 g piece of solid aluminum reacts with gaseous oxygen from the atmosphere to form solid aluminum oxide. In the laboratory, a student weighs the mass of the aluminum oxide collected from this reaction as 0.1798- 1st attempt Part 1 See Periodic Table The 0.156 g solid aluminum is the Choose one: A theoretical yield B. excess reagent C. percent yield D. actual yield E limiting reagent

Answer 1

Question The reaction of aluminium metal with Beygen can be written as gaseas mass: (8 molar mass: 0.156 that ething in the interior 4 Al 6) + 3% (2) 2 Al2O3 0.139 la mod) 269815 101.96 from the given data, it may be concluded aluminium metal will be the limiting real tant or and mixture. completely consumed in the . Atmospheric gas the excess neac tant According to stoichiometric ratio, moles of Al reacts = tar mass 0.1569 26.9815 g/mol = 0.0057zmoe 0.00578 mol Alx 2 mole Als us oxygen will be mass & Theoretical yield of Al2O3 (aluminium oxide) Ole Alz03 101.96g 01203 mole al a gield yield of Ala oz = 0.17 g х Actual 1 mole Alog - 0.2947 g of ol23 Perunt yield & Actual yield tical gera X 100). s o.179 a 0.29479 = 60.7397. Part 2 The 0.156 og solid aluminium is the limiting reagent Part-2 The o.179 g aluminium oxide is the 6 Actual yield. Part-3 The gaseous say gen is the ② Exass reagent Parten of this reaction The perunt yield 60.739).