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.

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.

The following redox reaction occurs in a galvanic cell. 2Al_((s))+3Fe_((aq))^(2+)(1M)rarr 2Al_((aq))^(3+)(1M)+3Fe : If E^@anode = -1.66 V and E^@cathode =-0.44 Calculate DeltaG^@ for reaction.

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.

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

Write the cell reaction and calculate the emf of the cell,at 25^@C, Cr(s)|Cr^3+(0.0065 M)|| Co^(2+)(0.012M)|Co(s), E_(Co)^0 =0.280 V, E_(Cr)^0 = 0.74V . What is DeltaG for the cell reaction ? std potential=0.4463v

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 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 .

Write the cell reaction and calculate the emf of the cell. Pb_((s))|Pb^(2+) (1M)||KCI(sat)|Hg_2CI_(2(s))|Hg E_(anode)^@=-0.126 V, E_(cathode)^@ = 0.242V . Identify anode and cathode. Name the right hand side electrode

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.