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Unformatted text preview: 3.55g = 34.00g 30.45g %Yield = Weight of Product Obtained * 100 Weight of Product Expected 55% = (3.55g/6.38g) * 100 Weight of Product Expected = (Moles of Fe(NH 4 ) 2 (SO 4 ) 2 *6H 2 O)* (1 Mole K 3 [Fe(C 2 O 4 ) 3 ]*3H 2 O ) *(MW of K 3 [Fe(C 2 O 4 ) 3 ]*3H 2 O) (1 Mole Fe(NH 4 ) 2 (SO 4 ) 2 *6H 2 O) 6.38g = (.013mol Fe(NH 4 ) 2 (SO 4 ) 2 *6H 2 O)*(1)*(492.1g/mol) Discussion: The obtained amount of the complex (3.55g) almost half of the expected value (6.38g). Possible reasons for this may be that some of the product was lost throughout the course of the experiment. This could have happened as it was being handled and emptied from one container to another. Ideally the % yield would be more than the 55% obtained....
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This note was uploaded on 04/17/2008 for the course CHEM 112 taught by Professor Hardy during the Spring '08 term at UMass (Amherst).
- Spring '08