Consider the following cell `Pb_((s))|Pb_((aq))^(2+)(0.5M)||Cu_((aq)^(+2)(0.001M)|Cu E^@Pb= -0.126V, E°Cu = +0.337V: Calculate `E_(cell) and `E_(cell)^@ at 25^@C`.

Consider the following cell Pb_((s))|Pb_((aq))^(2+)(0.5M)||Cu_((aq)^(+2) (0.001M)| E^@Pb = -0.126V E°Cu = +0.337V: Write the cell reaction.

Consider the following cell Pb_((s))|Pb_((aq))^(2+)(0.5M)||Cu_((aq)^(+2)(0.001M)|= -0.126V, E°u = +0.337V: Calculate DeltaG and DeltaG^@ for cell reaction.

Calculate emf of the following cell at 25^@C . Zn((s))|Zn^(2o+)(0.08M)||Cr^(3o+)(0.1M)|Cr E_(Zn)^0=-0.76V, E_(Cr)^0=-0.74V)

Calculate the standard cell potentials of galvanic cell in which the following reactions take place 2Cr_((s)) + 3Cd_((aq))^(2+)rarr 2Cr_(aq)^(3+) + 3Cd E_(Cr)^@ = -0.740 V, E_(Cd)^@ = -0.403 V, Calculate the Delta_rG^@ and equilibrium constant of the reactions.

Calculate the potential of the following cell at 25^@C . Sn_((s))|Sn^(2+) (0.025M)||Ag^+ (0.015M)|Ag(s) E_(sn)^0 = -0.136V, E_(Ag)^@ = 0.799V .

Consider the following redox reaction Mg_((s))+Sn_(aq)^(2+) rarr Mg_(aq)^(2+) +Sn_((s)) [Mg^(2+)] = 0.035M, [Sn^(2+)] = 0.025M , E_(Mg)^0 =- 2.37V and E_(Sn)^0 =-0.136V . Calculate DeltaG for the cell reaction.

Consider the following redox reaction Mg_((S)) +Sn_((aq))^(2+) rarr Mg_((aq))^(2+)+Sn_((s)) : Write the cell formula.

Write the Nernst equation and emf of the following cells at 298K. Mg_((s))| Mg_(aq)^(2+)(0.001M)| Cu_((s)) (Given E_(Mg^(2+)//Mg)^@ = -2.37 V, E_(Cu^(2+) //Cu)^@=0.34V)