Given: `E_(Sn^(2+)//Sn) ^0 = -0.14V` , `E_(Pb^(2+)//Pb) ^0 = -0.13V`. Determine `[(Sn^(2+))//(Pb^(2+))]` at equilibrium. For cell reaction `Sn |Sn^(2+) || Pb^(2+) | Pb` , Take `(2.303RT)//F = 0.06V`

For an electrochemical cell Sn(s)Sn^(2+) (aq,1M)||pb^(2+) (Aq,1M)|Pb(s) the ratio ([Sn^(2+)])/([Pb^(2+)] when this cell attians equilibrium is_______ (Given : E_(sn^(2+)|Sn)^(@) = -0.14V, E_(pb^(2+|Pb^(@))= -0.13V, (2.303RT)/(F = 0.06))

For an electrochemical cell Sn(s)|Sn^(2+)(aq, 1M)||Pb^(2+)(aq, 1M)|Pb(s) the ratio ([Sn^(2+)])/([Pb^(2+)]) when this cell attains equilibrium is _________________. ("Given "E_(Sn^(2+)|Sn)^(@)=-0.14V, " "E_(Pb^(2+)|Pb)^(@)=-0.13V,(2.303RT)/(F)=0.06)

Given : E^(@) (Cu^(2+//Cu) = 0.337V and E^(@) (Sn^(2+//Sn) = -0.136V . Which of the following statements is correct?

Calculate the equilibrium constant K_(c) for the rections. 3Sn^(4) + 2 cr to 3Sn^(2+) + 2Cr^(3+) Given E^(o) = 0.885 V .