What is the percent yield of a reaction in which 220 g of phosphorus trichloride reacts with excess water to form 122 g of HCl and aqueous phosphorous acid (H3PO3)?
PCl3 + 3H2O --------> H3PO3 + 3HCl
stoichimetric masss
PCl3 = 1mole×137.33g/mol = 137.33g
H2O = 3mole × 18 g/mol = 54g
H3PO3 = 1mole × 82g/mol = 82g
HCl = 3mole × 36.46 =109.38g
Actual mass of reactants
PCl3 = 220g
water = excess
Theoretical yield
stoichiometrically 137.33g of PCl3 give 109.38g of HCl
therefore, 220g of PCl3 should give
(109.38g/137.33g)×220g =175.22g of HCl
so , theoretical yield = 175.22g
percent yield
percent yield = (actual yield/theoretical yield) × 100
= (122g/175.22g)×100
= 69.63%
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