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Question

The standard electrode potential for an electrochemical cell is 2.2 V. Calculate the standard Gibbs energy change for reaction:
X(s)+Y2+(aq)X2+(aq)+Y(s)
(Given, 1F=96500 C mol1)
(correct answer +1, wrong answer -0.25)


A
554.632 kJ/mol
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B
384.786 kJ/mol
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C
424.6 kJ/mol
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D

384.123 kJ/mol

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Solution

The correct option is C 424.6 kJ/mol
X(s)+Y2+(aq)X2+(aq)+Y(s)
ΔGo=nFEo(cell)
n=2
F=96500 C mol1Eocell=2.2 V
ΔGo=2×2.2 V×96500 C mol1
ΔGo=424600 C V mol1
1 C V=1 Joule
ΔGo=424.600 kJ mol1

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