cuso4.5h20 + 2c2h5no2 = cu(gly)2.h20
moles of cuso4.5h2o produced is 12mmoles
moles of glycine poriduced is 16.5 mmoles.
which is the limiting reagent?
You need to rephrase this question. You have CuSO4.5H2O produced but it is a reactant. And I don't see where you have any glycine at all.
To determine the limiting reagent, you need to compare the number of moles of each reactant and their respective stoichiometric coefficients in the balanced chemical equation.
First, let's examine the balanced chemical equation for the reaction:
Cuso4.5H2O + 2C2H5NO2 -> Cu(gly)2.H2O
From the equation, the stoichiometric ratio between Cuso4.5H2O and Cu(gly)2.H2O is 1:1, and the stoichiometric ratio between C2H5NO2 and Cu(gly)2.H2O is 2:1.
Given that the moles of Cuso4.5H2O produced is 12 mmol, and the stoichiometric ratio is 1:1, we can conclude that the moles of Cu(gly)2.H2O produced is also 12 mmol.
Similarly, the moles of glycine produced is given as 16.5 mmol. Since the stoichiometric ratio between C2H5NO2 and Cu(gly)2.H2O is 2:1, we divide the moles of glycine by 2 to find the moles of Cu(gly)2.H2O produced from C2H5NO2:
16.5 mmol / 2 = 8.25 mmol
Now, we compare the moles of the two reactants: Cuso4.5H2O (12 mmol) and C2H5NO2 (8.25 mmol).
Since the moles of C2H5NO2 (8.25 mmol) are less than the moles of Cuso4.5H2O (12 mmol), the C2H5NO2 is the limiting reagent. This means that C2H5NO2 will be completely consumed in the reaction, and there will be some amount of Cuso4.5H2O left over.
Therefore, C2H5NO2 is the limiting reagent in this reaction.