What is the value for for the redox reaction shown E°cell below?
and is the reaction spontaneous?
Sn2+ (aq) + 2 Ag(s) → Sn(s) + 2 Ag+(aq)
a) -0.94 V
b) -0.66 V
c) +0.66 V
d) +0.94 V
Lets find Eo 1st
from data table:
Eo(Ag+/Ag(s)) = 0.80 V
Eo(Sn2+/Sn(s)) = -0.14 V
As per given reaction
cathode is (Sn2+/Sn(s))
anode is (Ag+/Ag(s))
Eocell = Eocathode - Eoanode
= (-0.14) - (0.80)
= -0.94 V
Answer: a
Since Eocell is negative, the reaction is not spontaneous
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