    Question

# The E0cell for the given cell reaction is −0.32 V at 25oC. Fe(s)+Zn2+(aq)⇌Zn(s)+Fe2+(aq) What will be the value of log[Fe2+] at equilibrium when a piece of iron is placed in a 1 M of Zn2+ solution?

A
10.83
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B
5.42
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C
+10.83
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D
+5.42
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Solution

## The correct option is A −10.83We have the Nernst equation at equilibrium at 25oC E0=0.0591nlog K......(Eqn.1) Since E0cell for the given reaction is negative, therefore, the reverse reaction is feasible for which E0cell will be +0.32 V. Thus, Zn(s)+Fe2+(aq)⇌Fe(s)+Zn2+(aq);E0cell=+0.32 V By Equation (1), we get E0=0.0591nlog[Zn2+][Fe2+] [Zn2+]=1 M 0.32=0.05912log1[Fe2+] 0.32=−0.05912log[Fe2+] log[Fe2+]=−10.829≈−10.83  Suggest Corrections  0      Similar questions  Explore more