Using the following Standars electrode potentials: Ag_(aq)^+ +e^- rightarrow Ag,

Question

Using the following Standars electrode potentials: Ag_(aq)^+ +e^- rightarrow Ag, E^degree: 0.80V Mn_(aq)^2+ + 2e^- rightarrow Mn; E^degree: 1.18V which of the following statement is Not correct for the standard cell shown below? Mn|Mn_(aq)^z+||Ag_(aq)^+| Ag Select one. The cell voltage will be 1.98 V the one cell reaction is Mn rightarrow Mn^z+ +2e^- the overall cell potential will decrease with time Ions migrate in the Solution, amp; electrons flow through the external Circuit Anions will be attracted to the Ag electrode compartment.

Explanation / Answer

Eo=reduction potential is high for Ag+/Ag half -cell=0.80 V

for Mn2+/Mn Eo=-1.18 so Ag+ will be reduced and form the cathode while Mn2+ will be oxidized and form anode.

Mn/Mn2+// Ag+/Ag

a)Eocell=Eored,cathode-Eo red,anode=0.80-(-1.18)=1.98V true

b)true oxidation of Mn

c)true

d)true

e)false ,Ag+(aq) are attracted ,cations

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