Nernst equation for Zn((aq))^(2+)+2e^(-)...

Nernst equation for `Zn_((aq))^(2+)+2e^(-) to Zn_((s))` is `E_(Zn^(2+)//Zn)` =__________.

`E_((Zn^(2+)//Zn))^(@)+(2.303RT)/(2F) log_(10) [Zn^(2+)]`

`E_((Zn^(2+)//Zn))^(@)-(2.303RT)/(2F) log_(10) [Zn^(2+)]`

`E_((Zn//Zn^(2+_)))^(@)+(2.303RT)/(2F) log_(10) [Zn^(2+)]`

`E_((Zn//Zn^(2+_)))^(@)-(2.303RT)/(2F) log_(10) [Zn^(2+)]`

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If [Zn^(2+)] is maintained at 1.0 M (i) What is the minimum (Cu^(2+)) for which the reaction Zn_((s))+Cu_((aq))^(2+) to Cu_((s))+Zn_((aq))^(2+) is still spontaneous in formward direction. (ii) Does the displacement of Cu_((aq))^(2+)" by "Zn_((s)) go to completion? E_(Zn^(2+)//Zn)^(0)=-0.76V E_(Cu^(2+)//Cu)=0.34V

Calculate the half cell potential at 298K for the reaction, Zn^(+2) + 2e^(-) rarr Zn " if " [Zn^(+2)] =2M, E_(Zn^(+2)//Zn)^(@) = -0.76V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V

Calculate the equilibrium constant for the reaction at 298 K Zn(s)+Cu^(2+)(aq)harr Zn^(2+)(aq)+Cu(s) Given " " E_(Zn^(2+)//Zn)^(@)=-0.76 V and E_(Cu^(2+)//Cu)^(@)=+0.34 V

Calculate E_("cell")^(0) of given electrochemical cell: Zn(s)+Cu^(2+) to Zn^(2+) (aq)+Cu(s) Given : E_(Zn^(2+)//Zn)^(0)=-0.76V E_(Cu^(2+)//Cu)^(0)=0.34V

Write Nernst equation for the following cell reaction : Zn(s) | Zn^(2+)(aq)|| Cu^(2+)(aq) | Cu(s)

Delta_rG^@ for the cell with the cell reaction : Zn_((s))+ Ag_2O_((s)) + H_2O_((l)) to Zn_((aq))^(2+) + 2Ag_((s)) + 2OH_((aq))^(-) [E_(Ag_2O // Ag)^(@)=0.344 V, E_(Zn^(2+)//Zn)^@=-0.76 V]

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