Question

need help figuring out 12 and 13, all of the questions

Cher 103A Electrochemistry -- which of the two diagrams below represents the galvanic cell? The electrolytic cell? How can you tell? Voltmeter Power supply Molten MX D a. For the galvanic cell if the cathode is on the left and the anode is on the right, which direction do the electrons flow? b. For the electrolytic cell in problem 4, where is the cathode, on the left or the right? Which direction do the electrons flow? Write the half reactions for MX in the electrolytic cell. 13. Consider the following galvanic cell: Fe(s) Fe(aq) || Ag (aq)| Ag(s)

Answer 1

Q:12 Ans :- First diagram in which two half cells (B and D) are connected with salt bridge (C) is Galvanic cell which convert chemical energy into electrical energy by spontaneous cell reactions.

Second diagram in which only one beaker is present is Electrolytic cell which convert electrical energy into chemical energy by non-spontaneous cell reactions.

(a). Direction of flow of electrons : Anode to Cathode i.e. E to A.

Q:13 Ans :- Representation of cell is : Fe (s) | Fe²⁺(aq) || Ag⁺(aq) | Ag(s)

(a). Positive (+) electrode is Cathode and Negative (-) electrode is Anode and U shaped tube which connect the two half cell is Salt bridge.

Direction of electrons it bridge ridge cathode. Facs) Anode Fecs) Salt 6 ครู 49)

(b).Reaction at Anode : Fe (s) ------------> Fe²⁺ (aq) + 2e^- , E⁰_Oxidation = + 0.45 V

Reaction at Cathode: 2 Ag⁺ (aq) + 2e^- ------------> 2 Ag (s) ,E⁰_Reduction = + 0.80 V

Adding both the half cell reactions, Overall cell reaction is :

Fe (s) + 2 Ag⁺ (aq) -------------------> Fe²⁺ (aq) + 2 Ag (s)

(c). Electrons flow from Anode to cathode while ions remains in the same container.

(d). Species present in anode = Fe and Fe²⁺ (aq)

Species present in cathode = Ag and Ag⁺ (aq) .

(e). Standard cell potential (E⁰_cell) = E⁰_Oxidation + E⁰_Reduction​​​​​​​ = 0.45 V + 0.80 V = 1.25 V

(f). ΔG⁰ = - n F E⁰_cell

Here, n= number of electron exchange in the reaction = 2

F = Faraday constant = 96500 C

ΔG⁰ = - (2) (96500 C) (1.25 V)

ΔG⁰ = - 241.250 KJ/mol