Need help.... calculate the theorectical yield of the compounds to be prepared in the experiment. The metal ion in both cases is the limiting reagent.Find number of moles of Cu(II) in the sample of CuSO4 x 5H2O that you used. The equal the number of moles of [Cu(NH3)4]x H2O that could theoretically be prepared. Proceed in a similar way for the synthesis invloving Co(II).
This what I got.
CuSO4 x 5H20
mass=3.86g
3.86/249.70g/mol=1.526x10-4 CuSO4
each mole CuSO4x5H20 will dissociate in 1 mole Cu2+ and 1 mol SO4 2-, giving a total of 2 moles of ions.
1.546x10-2 mols CuSO4 x 2= 3.09 x 10-2 mole ions
Also, how would i establish that the metal ion is the limiting reagent?
To calculate the theoretical yield of a compound, you need to determine the number of moles of the starting material and use stoichiometry to calculate the number of moles of the desired compound that could theoretically be formed.
For the CuSO4 x 5H2O compound:
1. Start by calculating the number of moles of CuSO4 x 5H2O used. You have the mass of the compound as 3.86g. You can convert this mass to moles by dividing it by the molar mass of CuSO4 x 5H2O, which is 249.70g/mol.
Moles of CuSO4 x 5H2O = 3.86g / 249.70g/mol = 0.0154 mol
2. In CuSO4 x 5H2O, each mole of the compound dissociates into 1 mole of Cu2+ and 1 mole of SO4 2- ions. This means that for every 1 mole of CuSO4 x 5H2O, you get a total of 2 moles of ions.
Moles of ions = Moles of CuSO4 x 5H2O x 2 = 0.0154 mol x 2 = 0.0309 mol
So, in this case, the number of moles of CuSO4 x 5H2O that you used is 0.0154 mol, and this would theoretically produce 0.0309 mol of ions (Cu2+ and SO4 2-).
To establish that the metal ion is the limiting reagent, you need to compare the number of moles of the metal ion (Cu2+ or Co2+) with the number of moles of the other reactant (ammonia or any other ligand).
For example, if you were testing with Cu2+ and [Cu(NH3)4]x H2O as the product:
1. Assume you have a certain number of moles of Cu2+ from the previous calculation (0.0309 mol in this case).
2. Determine the stoichiometry of the reaction between Cu2+ and ammonia to find the ratio between them.
Let's say the stoichiometry is as follows:
[Cu(NH3)4]2+ + 2NH3 -> [Cu(NH3)6]2+
This reaction shows that 1 mole of Cu2+ reacts with 2 moles of NH3 to produce 1 mole of [Cu(NH3)4]2+. So, the ratio is 1:2.
3. Compare the number of moles of Cu2+ with the number of moles of NH3 you have available. If the ratio of Cu2+ to NH3 is greater than 1:2, then Cu2+ is the limiting reagent. If it is less than 1:2, then NH3 is the limiting reagent.
Repeat this process for the synthesis involving Co(II) to determine the limiting reagent for that reaction as well.