Okay, I have a problem dealing with a pre-lab for aOxidation-Reduction Lab. The

Question

Okay, I have a problem dealing with a pre-lab for aOxidation-Reduction Lab. The lab is about starting with coppermetal and through a series of chemical reactions to recover thecopper and calculate the percent of recovery. My problem deals witha mathematical question pertaining to the lab. It reads:

"If nothing goes wrong and you start out with 0.211g copperturnings, what is the mass of copper compound that should beobtained in each step? Show your setups"
a. Cu(NO3)2
b. CuO
c. CuSO4

The five reactions are as follows:
1. Cu (s) +   4HNO3(conc) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)
2. Cu(NO3)2(aq) + 2NaOH (aq) -> Cu(OH)2(s) + 2NaNO3(aq)
3. Cu(OH)2(s) -> CuO(s) +   H2O(l)
4. CuO(s) + H2SO4(aq) -> CuSO4(aq) + H2O (1)
5. CuSO4(aq) + Zn(s) -> ZnSO4(aq) + Cu(s)

My question is how do you set up this particular problem and solveit. I seem to be stuck and cannot figure out what to do.Thanks.

Explanation / Answer

We solve this with stoichiometry! 0.211 grams of copper/1 x 1 mol /63.54 g is how we will begin every equation. I will outline how todo the first equation. Let's try #1. 0.211 grams of copper/1 x 1 mol of copper / 63.54 gCopper x 1 mol Cu(NO3)2/I mol Copper x 173.54 g Cu(NO3)2/1 molCu(NO3)2 = .576 grams of Cu(NO3)2. The trick is to use yourperiodic table to add the grams of each element contained in themolecule. For example, I added the molar mass of Cu with 2 Ns and 6Os to find this answer.

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