For the reaction `Fe(s) + Zn^(2+)(aq) rarr Fe^(2+)(aq) + Zn(s), E_(cell)^(@) = -0.32V`. What does the negative value of E' cell indicate?

The standard reduction potential of the half reaction Zn^(2+)(aq) + 2e^(-) rarr Zn(s), E^@ = 0.76V . What do you think of the standard reduction potential for the half reaction.

Depict the galvnic cell in which the reaction Zn(s) + 2Ag^+(aq) rarr Zn^(2+)(aq) + 2Ag(s) takes place. Further show: The carries of the current in the cell.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s) Also calculate the DeltarG^@ value of the reaction. (Given: E_(Cr^(3+)//Cr) = -0.74V , E_(Cd^(2+)//Cd) = -0.40V and F =96500C//mol )

The cell in which the following reactions occur: 2Fe_(aq)^(3+) + 2I_(aq)^(-) rarr 2Fe_(aq)^(2+) + I_(2(s)) has E_(cell)^@ = 0.236V at 298K.Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Fe^(3+)+e rarr Fe^(2+)_(aq) , E^@ = -0.77V Write the reaction which could be feasible using above half cells.

Depict the galvnic cell in which the reaction Zn(s) + 2Ag^+(aq) rarr Zn^(2+)(aq) + 2Ag(s) takes place. Further show: Which of the electrode is negatively charged?

The cell in which the following reaction occur. 2Zn(s)+2Cu^(2+)(aq) rarr 2Zn^(2+)(aq)+2Cu(s)E_(cell)^@=1.10 volt at 298K. Calculate the standard Gibbs energy and the equilibrium constant.

Complete the reaction Zn(s) + NaOH(aq) overset(Delta)rarr

Depict the galvnic cell in which the reaction Zn(s) + 2Ag^+(aq) rarr Zn^(2+)(aq) + 2Ag(s) takes place. Further show: Individual reaction at each electrode.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: Fe^(2+)(aq) + Ag^+(aq) rarr Fe^(3+)(aq) + Ag(s) . Calculate the Delta_rG and equilibrium constant of the reactions.