`E^@ (reduction potential) of Cu and Zn are +0.34V and -0.77V respectively. Which of them is stronger reducing agent?

Calculate the equilibrium constant for the reaction. 2Fe^(3+)+3I^-harr2Fe^2+I_3^- The standary reduction potentials in acidic conditions are 0.77V and 0.54V respectively for Fe^(3+)//Fe^(2+) and I_3^-//I^- couples.

The standard reduction potential values of three metal cations, X, Y and Z are +0.52, -3.03, -1/18V respectively. Arrange the corresponding metals in order of their increasing reducing power.

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.

The standard potential of Cu//Cu^(2+) electrodce = -3.34V. It corresponds to the raction

Represent the cell with cell reaction- Zn(s)+2Ag^+(aq) rarr Zn^(2+) (aq)+2Ag(s) Calculate the emf of the cell at 298K if the molar concentraction of Ag^+ and Zn^(2+) ions in the half cwells are 0.10 mol dm^(-3) and 0.01 mol dm^(-3) respectively. Given that E^@ Ag^+//Ag= 0.80V and E^@Zn^(2+)//Zn=-0.76V,

A copper silver cell is set up. The copper ion concentration is 0.10M . The concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. (Given) E_(Ag^(2+)//Ag)^@=+0.80V,E_(Cu^(2+)//Cu)^@=+0.34V

The standard electrode potential for Daniel cell is 1.1V. Calculate the standard Gibb's energy for the reaction. Zn_(s)+ Cu_(aq)^(2+) rarr Zn_(aq)^(2+)+Cu_(s) .