Question

Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 2.71×10−3.

Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 2.71×10−3.

Homework Answers

Answer #1

Solution :

Overall cell reaction is

X(s)+Y+(aq) -- > X+(aq)+Y(s)

n = Number of electrons involved =1

K = 2.71 E-3

We know

Delta G0 = - RTlnK

R = 8.314 J / (mol K )

T = 298.15 K (room T)

Ka is equilibrium constant for this reaction

Lets plug the values and get the Delta G0

Delta G0 = - [ 8.314 x 298.15 x ln (2.71 E-3)] J

= -(-14651.82 J )

= 14651.82 J

Now using it we get value of E0

Delta G0 = - nE0 F

Here Delta G0 is standard free energy change , n = number of electrons involved in overall reaction.

E0 standard electrode potential of cell. F is faraday’s constant value is 96500 C / mol

Lets find Delta G0

E 0 = - Delta G0/ n F

= - [14651.82 J / 1 x 96500 ] V

=- 0.152 V

So standard electrode potential of cell = 0.152 V

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