What is the standard cell potential for the voltaic cell?
`Cr || Cr^(3+) || Pb^(2+)|| Pb`
`{: ("Reaction", E_(red)^(@)//V), (Pb^(2+) + 2e^(-) rightarrow Pb, -0.13), (Cr^(3+) + 3e^(-) rightarow Cr, -0.74):}`

What is the standard cell potential for the reaction, 2Cr(s) + 3Sn^(2+)(aq) rightarrow 3Sn(s) + 2Cr^(3+)(aq) given the E^(@) values shown?

Find out work done for the given cell Cr| Cr^(+3)|| Fe^(+2)| Fe E_(Cr//Cr^(2+))^(@) = 0.74V, E_(Fe^(2+)//Fe)^(@) = -0.44V

What is the potential for the cell Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe E^(@)Cr^(3+)// Cr=-0.74V , E^(@)Fe^(2+)//Fe=-0.44V

What is the potential for the cell Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe E^(@)Cr^(3+)// Cr=-0.74V , E^(@)Fe^(2+)//Fe=-0.44V

What is the cell potential of the following cell ? Zn(s)|Zn^(2+)(1.0M)||Pb^(2+)(1.0M)|Pb(s) Given : E_(Pb^(2+)//Pb)^(@)=-0.12" V and " E_(Zn^(2+)//Zn)^(@)=-0.76" V"

Calculate standard cell potential of following galvanic cell Zn//Zn^(2)+(1 M) // Pb^(2)+(1 M)//Pb . If E_(Pb)^(0) = 0.126V and E_(Zn)^(0) = -0.763V

Write the cell reactions of the cell fored from Sn^(2+)//Sn, Pb^(2+)//Pb electrode E^(@)Sn^(2+)//Sn= -0.140V , E^(@)Pb^(2+)//Pb = -0.126V

Given these standards reduction potentials, what is the free energy change (in kJ. Mol^(-) for the reaction: Pb(s) + 2Ag^(+)(aq) rightarrow Pb^(2+)(aq) + 2Ag(s) Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.80V Pb^(2+)(aq) + 2e^(-) rightarrow Pb(s) E^(@) = -0.13V