Assume a cell with the following reaction {Cu}_{(s)}+2 {Ag}^{+}(1 \\times10^{-3} {M}) \\to{Cu}^{2+}(0.250 {M}) +2 {Ag}_{({s})} {E}^{⊝}_{\text{cell }} =2.97 {V} {E}_{\text{cell }} for the above reaction is __________ V. (Nearest integer) [ Given : \log 2.5=0.3979, {T}=298 {K}] [22 Jul 2021 Shift 2]

Electrochemistry Part 1

Section: Chemistry

Question : 10 of 100

Marks: +1, -0

Assume a cell with the following reaction
Cu(s)+2Ag+(1×10−3M)→Cu2+(0.250M) +2Ag(s)
Ecell ⊝=2.97V
Ecell for the above reaction is __________ V.
(Nearest integer)
[ Given : log‌2.5=0.3979,T=298K]

[22 Jul 2021 Shift 2]

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