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liberstina [14]
3 years ago
14

What is the value of ΔGo in kJ at 25 oC for the reaction between the pair: Mn(s) and Ag+(aq) to give Ag(s) and Mn2+(aq) Use the

reduction potential values for Ag+(aq) of +0.80 V and for Mn2+(aq) of -1.18 V Give your answer using E-notation with ONE decimal place
Chemistry
1 answer:
Leni [432]3 years ago
8 0

Answer:  -3.8\times 10^{5}J

Explanation:

Mn+2Ag^{+}\rightarrow Mn^{2+}+2Ag

Here Mn undergoes oxidation by loss of electrons, thus act as anode. silver 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_{[Mn^{2+}/Mn]}= -1.18V

E^0_{[Ag^{2+}/Ag]}=+0.80V

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

E^0=+0.80- (-1.18V)=1.98V

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

\Delta G^0=-nFE^0

\Delta G^0 = gibbs free energy

n= no of electrons gained or lost  = 2

F= faraday's constant

E^0 = standard emf  = 1.98V

\Delta G^0=-2\times 96500\times (1.98)=-3.8\times 10^{5}J

Thus the value of \Delta G^0 is -3.8\times 10^{5}J

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