Answer the following questions related to the given electrochemical cell under s

Question

Answer the following questions related to the given electrochemical cell under standard conditions.

1. Answer the following questions.

(a) The half cell containing W/W3+ is the  anode/ cathode

(b) Which one of the following statements is TRUE for the half cell containing W and W3+.
W3+ will be oxidized to form W.
W3+ will be reduced to form W.
W will be reduced to form W3+.
W will be oxidized to form W3+.

(c) The half cell containing Co2+/Co is the  anode/ cathode

(d) Which one of the following statements is TRUE for the half cell containing Co and Co2+.
Co will be reduced to form Co2+.
Co will be oxidized to form Co2+.
Co2+ will be reduced to form Co.
Co2+ will be oxidized to form Co.

2. What is E°cell (in V)? Report your answer to three decimal places in standard notation (i.e., 0.123 V).

3. Answer the following questions.

(a) Which one of the following is the balanced chemical equation for the spontaneous process occurring in the electrochemical cell under standard conditions?
3W3+(aq) + 2Co(s) 3W(s) + 2Co2+(aq).
2W(s) + 3Co2+(aq) 2W3+(aq) + 3Co(s).
3W(s) + 2Co2+(aq) 3W3+(aq) + 2Co(s).
2W3+(aq) + 3Co(s) 2W(s) + 3Co2+(aq).

(b) How many electrons are being transferred in this balanced chemical reaction?

(c) What is G° (in kJ/mol)? Report answer to three significant figures in scientific notation (i.e., 1.23e2 kJ/mol)

4. If the reaction was allowed to proceed, the mass of the W electrode will (increase /decrease ) and the mass of the Co electrode will (increase/ decrease ) . The [W3+] in solution will ( increase /decrease) and the [Co2+] in solution will (increase/ decrease)

5. The salt bridge contains K+ and Cl. As the cell is in operation the K+ ions will tend to migrate toward the (anode /cathode) and the Cl ions will tend to migrate toward the ( anode/ cathode) . This occurs to counter balance any loss of ( W^3+ /Co^2+ ) ions as they precipitate onto the (W /Co) electrode

Explanation / Answer

Dear Student,

W3+(aq) +3e- = W(s), Here Reduction Occurs as W3+ is oxidized (loses 3 electrons) to form W(s).

The half-reaction on the cathode where reduction occurs. also there is +ve potential value E° = 0.100 V

Co(s) = Co2+(aq) + 2e , Here Oxidation Occurs as Co(s) is reduced (gain 2 electrons) to form Co2+(aq)

The half-reaction on the anode where Oxidation occurs. there is a negetive potential value E° = -0.280 V

Balance eqution,

W3+(aq) + Co(s) = W(s)+  Co2+(aq)

3W3+(aq) + 2Co(s) 3W(s) + 2Co2+(aq).

Ecell=Ecathode-Eanode = 0.100 V-(-0.280 V)=0.380V

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