posted by 496935sd on .
A copper wire weighing 5.463g was dissolved in excess nitric acid, precipitated as copper(2)carbonate with excess sodium carbonate, and then converted tooo copper(2) sulfate pentahydrate using excess sulfuric acid. A student carrying out these reactions produced 20.021g of copper(2) sulphate pentahydrate. What was the students percentage yield?it is a 2 step process, come up with 2 reactions and do the stochiometric method twice.
I think the preferred way of writing CuCO3 is copper(II) carbonate and not copper(2) carbonate.
One mole of Cu is involved from beginning to end; therefore, moles Cu = 5.463 g/atomic mass Cu = ??
That will give you ?? moles (the same number) of CuSO4.5H2O.
Grams CuSO4.5H2O = moles CuSO4.5H2O x molar mass CuSO4.5H2O = xx. This is the theoretical yield.
%yield = (actual yield/theoretical yield)*100 = zz.
You will need to follow the directions. I don't know why you are to do the stoichiometry twice. You didn't write the hint so I don't know if there are instructions there, too. Finally, remember to round to the correct number of significant figures.
ooo srry the hint was that u have to do the method twice
and thank u soo much