Cu(s) | Cu^2+(10^(-4) M) || Ag^+(10^(-3) M) | Ag(s)

Cu(s) | Cu^2+(10^(-4) M) || Ag^+(10^(-3) M) | Ag(s)

전지 Cu(s) | Cu^2+(1.0×10^(-4) M) || Ag^+(1.0×10^(-3) M) | Ag(s)

E° = 0.46 V의 E_cell을 구하라.

> 산화 반쪽 반응: Cu(s) → Cu^2+(aq) + 2e^-

> 환원 반쪽 반응: 2Ag^+(aq) + 2e^- → 2Ag(s)

> 전체 산화-환원 반응: Cu(s) + 2Ag^+(aq) → Cu^2+(aq) + 2Ag(s)

---> n = 2

( 참고 https://ywpop.tistory.com/5351 )

Cu(s) + 2Ag^+(aq) → Cu^2+(aq) + 2Ag(s)

Q = [Cu^2+] / [Ag^+]^2

= (1.0×10^(-4)) / (1.0×10^(-3))^2

= 100

Nernst 식

E = E° – (0.0592 V / n) × logQ

= E° – (0.0592 V / n) × log([생성물]/[반응물])

( 참고 https://ywpop.tistory.com/2900 )

= 0.46 – (0.0592 / 2) × log(100)

= 0.4008 V

답: 0.40 V

[키워드] 네른스트 기준, redox Cu + 2Ag^+ → Cu^2+ + 2Ag, cell Cu + 2Ag^+ → Cu^2+ + 2Ag