[" Relative efficiency of the following cell is "],[84%],[A_((s))+B_((aq))^(2+)rightleftharpoons A_((aq))^(2+)+B_((s))Delta H=-285kJ],[" Then the standard electrode potential of the "],[" cell will be "]

Efficiency of the following cell is 84% A(s)+B_(aq)^(2+) + B(s), DeltaH^(@) = -285KJ The standard electrode potential of cell will be.

Efficiency of the following cell is 84% A(s)+B_(aq)^(2+) + B(s), DeltaH^(@) = -285KJ The standard electrode potential of cell will be.

The efficiency of a hypothetical cell is about 84% which involves the following reactions: A(s) + B^(2+)(aq) rightarrow A^(2+)(aq) _ B(s) DeltaH = -285kJ Then, the standard electrode potential of the cell will be: (Asume DeltaS = 0)

The efficiency of a hypothetical cell is about 84% which involves the following reactions: A(s) + B^(2+)(aq) rightarrow A^(2+)(aq) _ B(s) DeltaH = -285kJ Then, the standard electrode potential of the cell will be: (Asume DeltaS = 0)

Efficiency of a cell reaction under standard conditions, A_((s)) + B^(+) rarr A^(+) + B_(s), DeltaH^(@) = -300 kJ is 70% . The standard electrode potential of cell is :

The equilibrium constant of the reaction : A_((s))+2B_((aq))^(+)hArr A_((aq))^(2+)+2B_((s)): E_(cell)^(@)=0.0295V is :

Write the cell reaction for each of the following cells. Pt,H_(2)(g)|H^(+)(aq)|Ag^(+)(aq)|Ag(s)

Write the cell reaction for each of the following cells. Ni(s)|Ni^(2+)(aq)||Cu^(2+)(aq)|Cu(s).