A cell reaction is given as :
`A (s)+B^(2+)(aq)harrA^(2)(aq)+B(s)`
Equilibrium constant `(K_(c))` for the cell is 10. Calculate `E_(cell)^(@)`.

For a cell reaction: A(s)+2B^(+)(Aq)rarrA^(2+)(aq)+2B(s) the equilibrium constant is 1xx10^4 calculate E_(cell)^@ .

For a cell reaction : A (s) + 2 B^(+) (aq) to A^(2+) (aq) + 2 B(s) the equilibrium constant 1 xx 10^(4) . Calculate E_(cell)^(Theta) .

For the cell reaction, A(s) + 2B^(-)"(aq) rarr A^(2+) (aq) + 2B(s) , the value of Kc is 3.98 xx 10^(15) .Calculate E_(cell)^(@) at 298 K.

Calculating the thermodynamic equilibrium constant from the cell emf : The standard emf for the following galvanic cell is 0.46 V Cu(s)|Cu^(2+)(aq.)||Ag^(+)(aq.)|Ag(s) Calculate the equilibrium cosntant K_(C) for the reaction Cu(s)+2Ag^(+)(aq.)hArr Cu^(2+)(aq.)+2Ag(s) Strategy : Substitute the standard emf into the Equation (3.9) realting this quantity to the thermodynatmic equilibrium constant, K_(eq.). Solve K_(eq.). Note that K_(eq.). = K_(C^(.))

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

E^(@) for the electrochemical cell Zn(s) | Zn^(2+)1M (aq)|| Cu^(2+) 1M(aq)| Cu (s) is 1.10 V at 25^(@) C. The equilibrium constant for the cell reaction, Zn(s)+Cu^(2+) (aq.) rarr Zn^(2+) (aq.) + Cu(s) will be: