농도차 전지. Ag-AgCl [Cl^-] 0.0150 M [Cl^-] 2.55 M

농도차 전지. Ag-AgCl [Cl^-] 0.0150 M [Cl^-] 2.55 M

A voltaic cell is constructed with

two silver-silver chloride electrodes,

each of which is based on the following half-reaction:

AgCl(s) + e^- → Ag(s) + Cl^-(aq)

The two half-cells have [Cl^-] = 0.0150 M

and [Cl^-] = 2.55 M, respectively.

a. Which electrode is the cathode of the cell?

b. What is the standard emf of the cell?

c. What is the cell emf for the concentrations given?

d. For each electrode, predict whether [Cl] will increase,

decrease, or stay the same as the cell operates.

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[참고] 농도차 전지

[ https://ywpop.tistory.com/9626 ]

a. Which electrode is the cathode of the cell?

농도가 높은 쪽이 환원 전극 [ cathode, (+)극 ],

농도가 낮은 쪽이 산화 전극 [ anode, (–)극 ].

답: [Cl^-] = 2.55 M

b. What is the standard emf of the cell?

E°의 값은 0(zero) V이다,

산화 전극과 환원 전극이 동일하기 때문에.

답: 0 V

c. What is the cell emf for the concentrations given?

AgCl(s) + e^- → Ag(s) + Cl^-(aq)

---> n = 1

E = E° – (0.0592 V / n) log([묽은 농도]/[진한 농도])

= 0 – (0.0592 / 1) log(0.0150 / 2.55)

= 0.132 V

답: 0.132 V

d. For each electrode, predict whether [Cl] will increase,

decrease, or stay the same as the cell operates.

높은(진한) 쪽은 감소하고, 낮은(묽은) 쪽은 증가할 것이다,

언제까지? 양쪽 농도가 똑같아질 때까지.

답: [Cl^-] = 2.55 M, cathode 농도 감소,

[Cl^-] = 0.0150 M, anode 농도 증가.

[ 관련 예제 https://ywpop.tistory.com/16546 ]

The concentrations of chloride ion in the two compartments

are 0.0156 M and 1.55 M, respectively.

[키워드] Ag-AgCl 농도차 전지 기준, Ag-AgCl 농도 전지 기준