Given
`Fe^(2+)//Fe(s)=-0.44V,Ag^+//Ag(s)=+0.80V`.
Calculate total emf of the cell.

Following are the data of standard reduction half cell potentials of certain electrochemical cells. E_(Ag^(+)//Ag)^@ = 0.80V & E_(Cu^(2+)//Cu)^@ = 0.34V E_(Sn^(2+)//Sn)^@ =-0.14V & E_(Na^(2+)//Na)^@ = -2.73V Calculate the standard EMF of the cells.

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,

Represent the cell in which the following rection takes place. Mg(s) + 2Ag^+(0.01M)rarr Mg^(2+)(0.140M)+2Ag(s) Write the Nemst equation and calculate the emf if the cell at 298K . Given E_(cell)^Theta=3.17V

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.

A cell of emf 4V and internal resistance 0.5 is connected across a load resistance (i) 7.52, (ii) 11.50, calculate (i) the ratio of difference in emf of the cell and the potential drop across the load.(ii) the ratio of current in the two cases.

Calculate the equilibrium constant for the following reaction. Fe(s)+2Ag^+(aq) rarr 2Ag(s)+Fe^(2+)(aq) E_(Fe^(2+)//Fe)^@=-0.44V,E_(Ag^+//Ag)^=+0.80V .

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?

Given the standard electroge potentials. K^+//K= -2.93V,Ag^+//Ag=0.80V, Mg^(2+)//Mg=-2.37V . Arranges these metals in their decreasing order of oxidising power.

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.