The measured EMF at 298 K for the cell reaction, `Zn(s) + Cu^(2+)(1.0 M) rarr Cu(s) + Zn^(2+)(0.1M)` is 1.13 V. Calculate `E^(@)` for the cell reaction.

Explanation

Using Nernst equation, `E_("cell") = E_("cell")^(@) - (0.0591V)/(2) "log" ([Zn^(2+)])/([Cu^(2+)])`
Substituting values of `E_("cell")` (1.13V), concentration of `Zn^(2+)(0.1M)` and concentration of Cu(1.0M)
`1.13V= E_("cell")^(@) - (0.0591V)/(2) "log" (0.1)/(1.0) = E_("cell")^(@)- 0.0295V log 10^(-1) = E_("cell")^(@)+ 0.0295Vlog 10`
`E^(@) = 1.13V - 0.0295= 1.1V`