Theoretical and Percentage Yields - Moles

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Smoke_565
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If 1 mole of CuSO4.5H2O reacts with 2 moles of Glycine to form 1 mole of a Copper Complex product, what is the expected number of moles for the Copper Complex product?

Given:

Molar Mass of CuSO4.5H2O = 249.682g/mol
Molar Mass of Glycine = 75.067g/mol
Molar Mass of Copper Complex (Product) = 229.679 g/mol

Moles of CuSO4.5H2Oused = 0.0120
Moles of Glycine used = 0.0333 / 2 = 0.0167

Hence, CuSO4.5H2O is the limiting reagent.

Theoretical Yield of Copper Complex Product = 2.76 g
Actual Yield from Experiment of Copper Complex Product = 1.39 g

To find the expected number of moles of the Copper Complex Product is it simply the mass obtained from the actual yield (1.39) divided by the Molar Mass of the product (229.679) or is it the theoretical yield (2.76) divided by the Molar Mass of the product (229.679)?

I'm slightly confused as to what the expected number of moles of product should be. I'm getting 0.01202 (2.76/229.679) but I'm not sure if that is right as that is the same answer as the number of moles of the limiting reagent.
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Borek
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(Original post by Smoke_565)
I'm getting 0.01202 (2.76/229.679) but I'm not sure if that is right as that is the same answer as the number of moles of the limiting reagent.
Why should it be a problem? If stoichiometry tells you you get 1 mole of the product per 1 mole of the limiting reagent, why would you expect number of moles of product to be different from the number of moles of the reactant?
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