For a reaction:` A(s) + 2B ^(+) rarr A^(2+) +2 B (s). K_(aq)` has been found to be `10^(12)` The `E^(o)` cell is :

For a reaction A(s) + 2B^(+) rarr A^(2+)+2B(s). K_(c) has been found to be 10^(14) The E^(o) ""_(cell) is :

For a reaction A(s)+2B^(o+) rarr A^(2+)+2B K_(c) has been found to be 10^(12) . The E^(c-)._(cell) is

For the redox reaction Zn(s) + Cu^(2+) (0.1M) rarr Zn^(2+) (1M) + Cu(s) that takes place in a cell, E^(o)""_(cell) is 1.10 volt. E_(cell) for the cell will be:

For a reaction A (s) + B^(2+) rarr B(s) + A ^(2+) , at 25^(@) C E^(o) "" _(cell) = 0.2955 V. Hence, K_(eq) will be :

Given the equilibrium constant : K_(c) of the reaction : Cu(s) + 2Ag^(+)(aq) rightarrow Cu^(2+) (Aq) + 2Ag(s) is 10xx10^(15) , calculate the E_(cell)^(@) of this reaction at 298K . ([2.303 (RT)/(Ft) at 298K = 0.059V])

The equilibrium constant for the reaction Sr(s)+Mg^(+2)(aq)rarr Sr^(+2)(aq)+Mg(s) "is" 2.69xx10^(12)at25^(@)C "The" E^(@) for a cel made up of Sr//Sr^(+2) and Mg^(+2)//Mg half cells is

The equilibrium constant for a cell reaction, Cu(g) + 2Ag^+(aq) → Cu^(2+)(aq) + 2Ag (s) is 4 × 10^16 . Find E° (cell) for the cell reaction.

For the given reaction. 2A(s) +B(g) hArrC(g)+2D(s) +E(s) the degree of dissociation of B was found to be 20% at 300k and 24% at 500 k the rate of backward reaction

Celll equation : A + 2B^(+) rarr A^(2+) + 2 B A^(2+) + 2e rarr A E^@ = + 0.34 V and log_(10) K= 15. 6 at 300 K for cell reactions Find E^@ for B^(+) +e rarr B Given [( 2.303 RT)/(nF) =0.059] at 300 K .

Depict the galvanic cell in which the reaction : Zn(s)+2Ag^(o+)(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show : a. Which of the electrode is negatively charged ? b. The carriers of the current in the cell. c. Individual reaction at each electrode.