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Chemistry 2

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calculate the theorectical yield of the compounds to be prepared in the experiment. The metal ion in both cases is the limiting reagent.Find nuber 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
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.

Also, how would i establish that the metal ion is the limiting reagent?

  • Chemistry 2 -

    You have posted this a number of times and I see you haven't received any help. I've resisted because the post isn't clear to me.If you will go through and type in the missing words (two or three of them are missing or they are typos) I might be able to make sense of the question. My quick answer about limiting reagent is that I see no mention of amount of NH3. Without that someone must TELL you which is the limiting reagent; the problem does that.
    Here is a link that has nothing to do with copper ammine complex; however, it will show you how to calculate theoretical yield and percent yield.

  • Chemistry 2 -

    I am also facing this problem. The question is correctly asked. The amount NH3 is not given, but the problem states that the metal ion is the limiting reagent.

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