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.
Hint:
I think the preferred way of writing CuCO3 is copper(II) carbonate and not copper(2) carbonate.
Cu(s) ==>CuCO3==>CuSO4.5H2O.
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
To calculate the student's percentage yield, we need to compare the actual yield (the amount of copper(2) sulfate pentahydrate produced by the student) with the theoretical yield (the maximum amount of copper(2) sulfate pentahydrate that could be produced based on the starting mass of the copper wire).
Here's how we can approach this problem with the given information:
Step 1: Dissolution of Copper Wire
To find the amount of copper(2) carbonate formed, we need to determine the balanced chemical equation for the reaction between the copper wire and nitric acid.
Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2
Based on the balanced equation, we can determine the molar ratio between copper and copper(2) carbonate. Since copper(2) carbonate has a formula weight of 123.55 g/mol and the molar ratio between copper and copper(2) carbonate is 1:1, we can find the theoretical yield of copper(2) carbonate.
Step 2: Precipitation of Copper(2) Carbonate
To find the amount of copper(2) sulfate pentahydrate formed, we need to determine the balanced chemical equation for the reaction between copper(2) carbonate and sodium carbonate.
CuCO3 + Na2CO3 → CuCO3·Cu(OH)2 + 2NaNO3
Based on the balanced equation, we can determine the molar ratio between copper(2) carbonate and copper(2) sulfate pentahydrate. Since copper(2) sulfate pentahydrate has a formula weight of 249.68 g/mol and the molar ratio between copper(2) carbonate and copper(2) sulfate pentahydrate is 1:1, we can find the theoretical yield of copper(2) sulfate pentahydrate.
Step 3: Calculation of Percentage Yield
To calculate the percentage yield, we divide the actual yield (20.021g of copper(2) sulfate pentahydrate) by the theoretical yield (calculated in steps 1 and 2) and multiply by 100.
Percentage Yield = (Actual Yield / Theoretical Yield) * 100
By following these steps, you can calculate the student's percentage yield for the production of copper(2) sulfate pentahydrate.