An electrochemical cell is constructed such that on one side a pure nickel electrode is in contact with a solution containing ni2+ ions at a concentration of 3 × 10−3 m. the other cell half consists of a pure fe electrode that is immersed in a solution of fe2+ ions having a concentration of 0.1 m. at what temperature will the potential between the two electrodes be +0.140 v?

The temperature at which given potential between the two electrodes is attained is 331.13 K

Explanation:

The substance having highest positive potential will always get reduced and will undergo reduction reaction.

The half reaction follows:

Oxidation half reaction:  

Reduction half reaction:  

Net reaction:  

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the of the reaction, we use the equation:

Putting values in above equation, we get:

To calculate the temperature at which the reaction is taking place, we use the Nernst equation, which is:

where,

= electrode potential of the cell = +0.140 V

= standard electrode potential of the cell = +0.19 V

n = number of electrons exchanged = 2

R = Gas constant = 8.314 J/mol.K

F = Faraday's constant = 96500

T = temperature of the reaction

Putting values in above equation, we get:

Hence, the temperature at which given potential between the two electrodes is attained is 331.13 K

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