In: Chemistry
A student started a synthesis of alum with 3.4x10^-2 mole aluminum:
2Al (s) + 6h2O (I) + 2KOH (aq)------> 2K[Al(OH)4] (aq) + 3H2 (g) (1)
2K[Al(OH)4] (aq) + H2SO4 (aq) ------> 2Al(OH)3 (s) +2 K2SO4 (aq) + 2H2O (I) (2)
2Al(OH)3 (s) + 3H2SO4 (aq) ---------> Al2(SO4)3 (aq) + 6H2O (3)
Al2(SO4)3 (aq) + K2SO4 (aq) + 24 H2O---------> 2KAl(SO4)2 12H2O (4)
a) What theoretical yield of alum, in gram, would be produced from 3.4x10^-2 mole of aluminum?
b) A student obtained 12.4 g alum from the synthesis. If the theortical yield was 19.6 g, what was the percent yield?
Ans. a. From the stoichiometry of equation 1 through 4-
2 moles of aluminum produce 2 moles of alum.
Thus, 3.4 x 10-2 moles of aluminum produce 3.4 x 10-2 moles of alum.
Molecular mass of alum = 474.39 gm/ mol
Theoretical yield of alum (g) = moles of alum x molecular mass of alum
=3.4 x 10-2 moles x 474.39 gm/ mol
= 16.13 gm
Ans. b. % yield = (yield obtained / theoretical yield) x 100
= (12.4 gm / 19.6 gm) x 100
= 63.27 %