Can we use a Copper Vessel to store 1M `AgNO_3` solution? Given that `E_(Cu^(2+)//Cu)^@ = 0.34v` and `E_(Ag^(+)//Ag)^@ = 0.80v`

Write the Nernst equation and calculate the emf of the following at 298K. Cu(s)|Cu^(2+)(0.13M)||Ag^+(1xx10^-4M)|Ag(s) Given E_(Cu^(2+)//Cu)^@ = 0.34V and E_(Ag^+//Ag)^@ = 0.80V

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknonw concentration. It other half cell consists of a zinc electrode dipping in 1.0M solution of Zn(NO_3)_2 . A voltage of 1.48V is measure for this cell. Use this information to calculate the concentration of silver nitrate solution used (E_(Zn^(2+)//Zn)^0=-0.76V,E_(Ag^+//Ag)^0=+0.80V)

Which is a stronger reducing agent Zn or Fe? If E_(Zn^(2+)//Zn)^@ = -0.76V , and E_(Fe^(2+)//Fe = -0.44V

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.

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)^@ = -2.74V Also identify andode, cathode and direction of flow of current in each of the constructed cells.

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)^@ = -2.71V Represent the electrochemical cell constructed from these pair of half cells.

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 )

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

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 .

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,