The cell in which the following reaction occurs
`2Fe^(3+)(aq)+2I-(aq) to 2Fe^(2+)(aq) + I_2(s)`
has `E_(cell)^0` = 0.236V at 298 K. Calculate the standard Gibbs energy and equilibrium constant of the cell reaction

Calculate the standard cell.potentials of galvanic cell in which the following reactions take place: Fe^2+(aq)+Ag+^*(aq)^* -> Fe^3+(aq)+Ag(s) Calculate the Delta r G^circ and equilibrium constant of the reactions.

Daniellcell converts the chemical energy liberated during the redox reaction to electrical energy. Zn_(s)+Cu_(aq)^(2+) rarr Zn_(aq)^(2+)+Cu_(s), E_(cell)^0=1.1V .Calculatethe standard Gibbs energy ( Delta_rG^0 ) for the reaction.

Represent the galvanic cell in which the reaction Is: Zn(s)+Cu^(2+) (aq) rarr Zn^(2+) (aq)+Cu(s)

Balance the following redox reaction by ion electron method MnO_4^- (aq) + I^- (aq) to MnO_2 (s) + I_2(s) (base medium)

The equilibrium constant for the following reaction at 298K is expressed as x xx 10^(y) . 2Fe^(3+) + 2I^(-) rarr 2Fe^(2+) + I_(2), E_("cell")^(@) = 0.236V . The value of y is …..

Write the half reaction for the following redox reaction. 2Fe^(3+)(aq) + 2l (aq) rarr I_2 (s) + 2Fe^(2+) (aq)

Balance the following redox reaction by ion electron method H_2O_2 (aq) + Fe^(2+) (aq) toFe^(3+)(aq) + H_2O (l) (acid medium)

Two electrochemical cells are assembled in which the following reaction occur. V^2+VO^2+2H^+ to 2V^3+H_2O, E_(cell) ^@=0.616V V^3+Ag^+ +H_2O to VO^2+2H^+ + Ag(s), E_(cell)^@=0.439V calculate E^@ for the half cell reaction V^(3+) +e to V^(2+) (E_(Ag)^@, Ag=0.799 volt )

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.

The equilibrium constant of the following redox reaction at 298 K is 1 xx 10^(8) 2Fe^(3+) (aq.)+ 2I^(-) (aq.) rarr 2Fe^(2+) (aq)+I_(2) (s) If the standard reduction potential of iodine becoming iodide is +0.54 V. What is the standard reduction potential of (Fe^(3+))/(Fe^(2+)) ?