The standard cell potential (e°cell) for the reaction below is +1.10v. the cell potential for this reaction is v when the concentration of [cu2+]=1.0⋅10−5m and [zn2+]=2.5m. zn (s) + cu2+ (aq) → cu (s) + zn2+ (aq) the standard cell potential () for the reaction below is . the cell potential for this reaction is when the concentration of and (s) + (aq) (s) + (aq) 0.78 1.10 0.94 1.26 1.42

0.94 V

Explanation:

For the given chemical reaction :

Using Nernst equation :

where,

F = Faraday constant = 96500 C

R = gas constant = 8.314 J/mol.K

T = room temperature =

n = number of electrons in oxidation-reduction reaction = 2

= standard electrode potential of the cell = +1.10 V

= emf of the cell = ?

Now put all the given values in the above equation, we get:

The cell potential for this reaction is 0.94 V

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