If you see electrode potential table , it shows that the one which having higher

Question

If you see electrode potential table , it shows that the one which having higher reduction potential will get reduced first:

EoCell = Eocathode - Eoanode

Eocathode = cathode reduction potential , or the one with higher reduction potential(will get reduced)

Eoanode = anode reduction potential , or the one with lower reduction potential

If you see reaction 1 and 2 , the one with higher reduction potential will work as cathode

EoCell = 0.54 - (0.28) = 0.82 V

If you see the bottom two

2 and 3

EoCell = 0.54 - (0.34) = +0.20 V

balanced reaction is :

cathode :

I2(s) + 2e- ----->2I-(aq)

anode:

Co(s) ------->Co2+(aq) + 2e-

add cathode and anode half reaction

I2(s) + Co(s) ----->2I-(aq) + Co2+(aq)

G = -nFEocell

n = no. of electron transfer

F = faraday's constant

G = -2 x 96500C x 0.82 V = -158260 J

Explanation / Answer

for this question, why won't the bottom 2 work as opposed to the top 2? I'm so confused

Given the following half-reactions, combine the two that give the cell reaction with the most positive E. Write a balanced equation 18.84 for the cell reaction, and calculate Ec and G. Co-Taq)-2 e--Co(s) E"=-0.28 V L(s) +2e 2r(aq) 0.54 V Cu2+(aq) + 2 e-_ Ca(s) E" = 0.34 V

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