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Question

Calculate the equilibrium constant for the redox reaction at 25oC, Sr(s)+Mg2+(aq)Sr2+(aq)+Mg(s), that occurs in a galvanic cell. EoMg2+/Mg=2.37V and EoSr2+/Sr=2.89V.

A
2.69×1015
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B
2.69×1017
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C
3.69×1017
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D
3.69×1015
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Solution

The correct option is C 3.69×1017
(i) Mg2+(aq)+2eMg(s);EoMg2+/Mg=2.37V
Sr2+(aq)+2eSr(s);EoSr2+/Sr=2.89V
(ii) Sr(s)Sr2+(aq)+2e;EoSr/Sr2+=2.89V

Adding (i) & (ii), we get,
Sr(s)+Mg2+(aq)Sr2+(aq)+Mg(s);Eo=2.37+2.89=0.52V
Now, ΔGo=RTlnKeq
nFEo=RTlnKeq
lnKeq=nFEoRT=2×96500×0.528.314×298
lnKeq=40.507
Keq=3.69×1017

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