1. I suggest you think of the various compounds of copper and ask yourself how you distinguish between them. The question is ambiguous to begin with because it doesn't specify by physical means or chemical means.
2. Again, if you synthesized these compounds you must have seem what they look like. Compare them with the (II) analogs and you have your answer.
3. How many grams do you if Cu? That's
mols Cu(NO3)2 = M x L = ?
mols Cu = the same since there is 1 mol Cu in 1 mol Cu(NO3)2.
Grams Cu = mols Cu x atomic mass Cu = ? This is the theoreticalyield (TY)
% recovery. You need to know how much Cu you recovered. Call that actual yield (AY). Then
% recovery = (AY/TY)*100 = ?
4. I don't understand 4.
word equation. There isn't a reaction in your example but it does dissolve so I would write it this way.
hydrochloric acid + copper(II) ==> copper 2+ ion(aq) + oxide ion(aq) + hydrogen ion(aq) + chloride ion(aq).
For a real reaction like this,
2HCl(aq) + CuS(s) ==> H2S(g) + CuCl2(aq)
hydrochloric acid + copper(II) sulfide yields hydrogen sulfide gas + copper(II) chloride
1. is it easy to distinguish between between the different oxidation states of copper? why?
2. You synthesized copper (I) chloride and copper (I) oxide. How do they differ from their copper (II) analogs? comment on the stability of these moist solids in air. If unstable, what is the likely product of decomposition?
3. calculate the percent recovery of copper from 10 mL of .10M of Cu(NO3)2? (how would you do this question?)
4. Is it necessary to synthesize the various copper compounds in order to recover copper metal?
Also, how can you write word equations for reactions? For example, adding HCl to CuO.
Any help with these questions would be greatly appreciated! even telling me how to go about them!!! thank you!!!
1 answer
0 answers