Galvanic Cell Lab AnodeCathode electrolyteObserved value At the anode side, ever

Question

Galvanic Cell Lab AnodeCathode electrolyteObserved value At the anode side, every zinc atom loses two electrons which can form aqueous Zn; At the cathode side, there will release hydrogen. Zn Zn(NO HydrogenHCI 0.76 At the anode side, every zinc atom loses two electrons which can form form solid copper, and the solid cooper will plate out on the cathode. At the anode side, every zinc atom loses two electrons which can form Zn Zn(NOCu 1.10 aqueous Zn2; At the cathode side, reduction occurs. The Cu in solution to Zn Zn(NOAg AgNOj 1.56 aqueous Zn2; At the cathode side, reduction occurs. The Ag in solution to form solid silver, and the solid silver will plate out on the cathode. At the anode side, every hydrogen atom loses one electron which can form hydronium ion into solution; At the cathode side, reduction occurs. The Cu in solution to form solid copper, and the solid cooper will plate out on the HydrogenHCI Cu Cu(NO0.34 At the anode side, every hydrogen atom loses one electron which can form solution to form solid silver, and the solid silver will plate out on the cathode. At the anode side, every cooper atom loses two electrons which can form form solid silver, and the solid silver will plate out on the cathode. HydrogenHCI Ag AgNO, 0.80 hydronium ion into solution; At the cathode side, reduction occurs. The Ag in Cu Cu(NOAg AgNO 0.46 aqueous CuAt the cathode side, reduction occurs. The Ag in solution to

Explanation / Answer

answers)

Here From the above given data

1. The net ionic equations are

Zn(s) + 2H+(aq) --> Zn2+(aq) + H2(g)

Zn(s) + Cu2+(aq) --> Zn2+(aq) + Cu(s)

Zn(s) + 2Ag+(aq) --> Zn2+(aq) + 2Ag(s)

H2(g) + Cu2+(aq) ---> 2H+(aq) + Cu(s)

H2(g) + 2Ag+(s) ---> 2H+(aq) + 2Ag(s)

Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s)

2.

the cell notations are

Zn(s) | Zn2+(aq) || HCl(aq) | H2(g)

Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s)

Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s)

H2(g) | HCl(aq) || Cu2+(aq) || Cu(s)

H2(g) | HCl(aq) || Ag+(s) | Ag(s)

Cu(s) | Cu2+ || Ag+(aq) | Ag(s)

3.

The Electric potentials are

Zn(s) + 2H+(aq) --> Zn2+(aq) + H2(g):

Eo = 0 - (-0.763) = 0.763 V

Zn(s) + Cu2+(aq) --> Zn2+(aq) + Cu(s)

Eo = 0.337 - (-0.763) = 1.100 V

Zn(s) + 2Ag+(aq) --> Zn2+(aq) + 2Ag(s)

Eo = 0.80 - (-0.763) = 1.563 V

H2(g) + Cu2+(aq) ---> 2H+(aq) + Cu(s)

Eo = 0.337 - 0 = 0.337 V

H2(g) + 2Ag+(s) ---> 2H+(aq) + 2Ag(s)

: Eo = 0.80 - 0 = 0.80 V

Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s) :

Eo = 0.80 - 0.337 = 0.463 V

4.

Here The observed value matches well with the calculate electric potential values.

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