What is the `E^(@)` value for the voltaic cell constructed from the half-cells?
`{: ("Reaction", E^(@)(V)), (Zn^(2+) + 2e^(-) rightarrow Zn,-0.762), (Tl^(+) + 3e^(-) rightarrow Tl, -0.036):}`

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):}

Which expression gives the correct value of the standard potential for a gold-rhodium voltaic cell? {:("Half-reaction",E^(@)V), (Rh^(3+)(aq) +_ 3e^(-) rightarrow Rh(s), 0.76), (Au^(+)(aq) + e^(-) rightarrow Au(s), 1.69):}

Use the information in the table and calcualate E^(@) for this reaction. Ga(s) + 3Tl^(+)(aq) rightarrow 3Tl(s) + Ga^(3+) (aq) {: ("Reaction", E^(@)), (Ga^(3+)(aq) + 3e^(-) rightarrow Ga(s), -0.529V), (Tl^(+)(aq) + e^(-) rightarrow Tl(s), -0.336V):}

For a galvanic cell involving the half-reaction at standard conditions, Au^(3+) + 3e(-) rightarrow Au E^(@) = 1.50V Tl^(+) + e(-) rightarrow Tl E^(@) = -0.34V

Calculate the half cell potential at 298K for the reaction, Zn^(+2) + 2e^(-) rarr Zn " if " [Zn^(+2)] =2M, E_(Zn^(+2)//Zn)^(@) = -0.76V

If [Zn^(2+)] = 0.1 M and E^(@) = -0.76 V then half cell potential at 298 K for the reaction Zn_((aq))^(2+)+2e^(-) rarr Zn_((s)) is

Which of the half reactions, when coupled, will make a galvanic cell that will produce the largest voltage under standard conditons? P. Cu^(2+)(aq) + 2e^(-) rightarrow Cu(s) E^(@) = +0.34V Q. Pb^(2+)(aq) + 2e^(-) rightarrow Pb(s) E^(@) = -0.13V R. Ag^(+)(aq) + 3e^(-) rightarrow Al(s) E^(@) = -1.66V

What is the standard potential of the Tl^(3+)//Tl electrode ? Tl^(3+)+2e^(-) rarr Tl^(+)," "E^(@)=1.26" volt" Tl^(+)+e^(-) rarr Tl," "E^(@)=-0.336" volt"