Using construct a standard electrochemical cell a strip of copper, a strip of zi

Question

Using construct a standard electrochemical cell a strip of copper, a strip of zinc, a solution of copperI) sulfate, and a solution of zinc sulfate by manipulating the standard reduction reactions below Zn2.aal + 2e Znisi a) Give the balanced half reactions. the balanced overall standard cell reaction and calculate the ·1 value Bal. Anode rxn: Bal. Cathode rxn: Bal. Overall rxn. b) How many moles of electrons flow in the balanced, overall cell reaction? How do you determine this? c) Is the cell spontaneous or nonspontaneous? d) What are the concentrations of all electrolytes in this standard cel? e) Give the line-notation of this electrochemical cell showing phase labels as well. Write the nots on provided "battery case" showing proper anode and cathode positions f) Write out the Q expression for the balanced cell reaction assuming an equilibrium exists: Electrolytic Galvanic g) This cell is (circle one):

Explanation / Answer

a)

anode : Zn (s) --------------------> Zn+2 (aq) + 2e- , Eo = -0.76 V

cathode : Cu+2 (aq) + 2e- -----------------> Cu (s) , Eo = + 0.34 V

overall reaction : Zn + Cu+2 -----------------> Zn+2 + Cu , Eocell = 1.10 V

b)

2 moles of electrons

c) yes . it is spontaneous

because Eocell is positive

d) concentrations = 1.0 M

e)   Zn(s) / Zn+2 (aq) // Cu+2 (aq) / Cu (s)

f) Q = [Zn+2] / [Cu+2]

g) galvanic cell

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