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

Which is a stronger reducing agents Cr^(2+) or Fe^(2+) and why?

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.

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

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 )

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)

Calculate e.m.f. of the following cell at 298K: 2Cr(s) + 3Fe^(2+)(0.1M) rarr 2Cr^(3+)(0.01M) + 3Fe(s) E^0 (Cr^(3+)/Cr) = -0.074V & E^0 (Fe^(2+)/Fe)= -0.44V

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