A chemist isolates 17.43 g of product from a reaction that has a calculated theoretical yield of 21.34 g. What is the percentage yield?© BrainMass Inc. brainmass.com October 24, 2018, 7:01 pm ad1c9bdddf
This solution calculates the percentage yield of a product from a reaction that has a theoretical yield of 21.34g.
Percent Yields and Limiting Reagents : NiCl2.6H2O + Ethylenediamine ---> Ni(en)3 Cl2
Some backround data:
mass of NiCl2 + 6H2O = 3g
mass of Ethylenediamine used: 2.85g
initial moles ethylenediamine: .0474 (I think)
product formed: mass of Ni(C_2_H_8_N_2_)_3_CL_2_: 3.597
The questions I need answered:
-theoretical moles of product, based on stoichiometry.
-molecular mass of product
-theoretical mass of product formed
-actual mass of product collected (I would assume that it is 3.597)
-percent yield of product.
Can the percent yield be increased by increasing the amount of the limiting reagent. Be sure to explain relationship between limiting reagent and theoretical yield and theoretical yield and percent yield, and to identify three things which could occur experimentally and lead to a yield of less than 100% of theoretical yield.
2. What might account for a calculated % yield greater than 100%?
Address the following:
-the solution volume containing dissolved nickel chloride is found to be greater than the amount of water added to dissolve it. explain this result.
-Ethylenediamine is colorless. In half of the reaction mixtures studied nickel chloride hexahydrate was limitng reagent, meaning that ehtylenediamine was in excess, however, none of the filtrates were colorless. What accounts for the observation?
keywords: nickel (II) chlorideView Full Posting Details