An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)→Sn2+(aq, 1.65 M )+2e− Red:...

An electrochemical cell is based on the following two half-reactions:

Ox: Sn(s)→Sn2+(aq, 1.65 M )+2e−

Red: ClO2(g, 0.165 atm )+e−→ClO−2(aq, 1.90 M )

Compute the cell potential at 25 ∘C.

Solutions

Expert Solution

Ans:- Compute the cell potential at 25 ∘C.

Ox: Sn(s)→Sn2+(aq, 1.65 M )+ 2e− : E = -0.14v

Red: ClO2(g, 0.165 atm )+ e−→ClO−2(aq, 1.90 M): E = 0.954v

E⁰ = E_C - E_A

= 0.954-(-0.14)

= 1.094v

NERNST EQUTION: E = E⁰ -0.0591/2*log (cathode)/(anode)

E = 1.094-0.029*log(1.90)²/(1.65)

E = 1.094-0.029*log 2.1878

E = 1.094-0.029*0.34

E = 1.0842 Volts

queen_honey_blossom answered 3 months ago

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