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The mass of the CuSO4 x 5H2O sample is 1.664 g. The mass of the recovered copper is 1.198 g.

1. Compute the experimental percent by mass of copper in the sample:
1.1664/1.998x 100=71.81%

2. Calculate the percent copper in pure copper sulfate pentahydrate(this is the theoretical percent copper). One mole of copper has a mass of 63.55 g, and by addition, one mole of CuSO4 x 5H2O has a mass of 249.5 g:

63.55/249.5x100= 25.47%

3. In order to calculate the error of the % Cu and the percent error of the % Cu I know I am suppose to use 1.198 as the experimental value, but I am not sure what to use for the true value.

  • chem - ,

    Something is haywire here.
    mass sample = 1.664 g.
    mass recovered Cu = 1.198 g.
    percent Cu = (1.198/1.664)*100 = 71.995 which I would round to 72.00 to four s.f.
    I don't know where you obtained 1.1664 nor 1.998. Check my work.

    For percent error.
    [(exp value - theoretical value)/theoretical value]*100 = ??
    The 25.47% is the theoretical value; i.e., what it's supposED to be.

  • chem - ,

    A mixture of two metals is analyzed by reacting it with dioxygen to completely convert the metals to their oxides. When 1.4850 grams of a nickel/chromium mixture is reacted, it produces 2.0759 grams of a mixture of Cr203 and NiO. What is the mass percent for each metal in the original mixture? Please help!

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