To find the standard potential of M3+/M electrode, the following cell is constituted : Pt/M/M3+(0.001molL−1)/Ag+(0.01molL−1)/Ag The emf of the cell is found to be 0.421 volt at 298 K The standard potential of half reaction M3+3e−→M at 298 K will be : (Given EeAg+/Ag at 298 K =0.80 Volt)
0.32 Volt
0.66 Volt
1.28 Volt
0.38 Volt
A
0.32 Volt
B
0.66 Volt
C
1.28 Volt
D
0.38 Volt
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Solution
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The correct option is A 0.32 Volt Ecell=E0cell−0.0592nlog[M3+][Ag+]3 0.421=E0cell−0.05923log0.001(0.01)3 E0cell=0.48V E0cell=E0Ag−E0M 0.48=0.80−E0Ag E0Ag=0.32 V The standard potential of half reaction M3+3e−→M at 298 K at 298 K will be 0.32 V.
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Similar Questions
Q1
To find the standard potential of M3+/M electrode, the following cell is constituted : Pt/M/M3+(0.001molL−1)/Ag+(0.01molL−1)/Ag The emf of the cell is found to be 0.421 volt at 298 K The standard potential of half reaction M3+3e−→M at 298 K will be : (Given EeAg+/Ag at 298 K =0.80 Volt)
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Q2
To find the standard potential of M3+|M electrode, the following cell is constituted: Pt|M|M3+(0.0018mol−1L)∥Ag+(0.01mol−1L)|Ag The emf of this cell is found to be 0.42volt. Calculate the standard potential of the half reaction M3++3e−→M. E∘Ag+/Ag=0.80volt.
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Q3
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The emf of the given cell is found to be 0.42V at 25∘C. Calculate the standard potential of the half reaction. M3+(aq)+3e−→M(s)
Given: E0Ag+/Ag=0.80V
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Q5
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