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NemiM [27]
3 years ago
9

What is the value of the equilibrium constant at 25 oC for the reaction between the pair: Ag(s) and Ni2+(aq) to give Ni(s) and A

g+(aq) Use the reduction potential values for Ag+(aq) of +0.80 V and for Ni2+(aq) of -0.25 V Give your answer using E-notation with NO decimal places
Chemistry
1 answer:
rusak2 [61]3 years ago
6 0

Answer: 3\times 10^{35}

Explanation:

The balanced chemical equation will be:

2Ag(s)+Ni^{2+}(aq)\rightarrow 2Ag^{+}(aq)+Ni(s)

Here Ag undergoes oxidation by loss of electrons, thus act as anode. Nickel undergoes reduction by gain of electrons and thus act as cathode.

E^0=E^0_{cathode}- E^0_{anode}

Where both E^0 are standard reduction potentials.

E^0_{[Ag^{+}/Mg]}=+0.80V

E^0_{[Ni^{2+}/Ni]}=-0.25V

E^0=E^0_{[Ni^{2+}/Ni]}- E^0_{[Ag^{+}/Ag]}

E^0=-0.25-(+0.80V)=-1.05V

The standard emf of a cell is related to Gibbs free energy by following relation:

\Delta G=-nFE^0

\Delta G = gibbs free energy  

n= no of electrons gained or lost  =?

F= faraday's constant

E^0 = standard emf

\Delta G=-2\times 96500\times (-1.05)=202650J

The Gibbs free energy is related to equilibrium constant by following relation:

\Delta G=-2.303RTlog K

R = gas constant = 8.314 J/Kmol

T = temperature in kelvin =25^0C=25+273=298K

K = equilibrium constant

\Delta G=-2.303RTlog K

+202650=-2.303\times 8.314\times 298\times logK

K=3\times 10^{35}

Thus the value of the equilibrium constant at 25^0C is 3\times 10^{35}

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