If △G∘ for the half cell MnO−4|MnO2 in an acid solution is xF then find the value of x. (Given: E∘MnO−4|Mn2+=1.5V;E∘MnO2|Mn2+=1.25V)
−0.75
−0.95
None of these
−0.85
A
−0.75
B
−0.95
C
−0.85
D
None of these
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Solution
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The expression for the standard free energy change is ΔG0=−nFE0 But it is equal to xF. Hence, x=−nFE0F=−nE0 But for the given half reaction, n=3 and E0=E0MnO−4|Mn2+−E0MnO2|Mn2+1.5−1.25=0.25V Hence, x=−nE0=−3×0.25=−0.75
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If △G∘ for the half cell MnO−4|MnO2 in an acid solution is xF then find the value of x. (Given: E∘MnO−4|Mn2+=1.5V;E∘MnO2|Mn2+=1.25V)