Given the standard reduction potentials, which statement is correct?
`{:(Cu^(2)(aq) + 2e^(-) rightarrow Cu(s), E^(@) = 0.34V), (2H^(+)(aq) + 2e^(-) rightarrow H_(2)(g), E^(@)= 0.0V), (Cr^(3+)(aq) + 2e^(-) rightarrow Cr(s),E^(@) = -0.73V):}`

Given these standard reduction potentials, what is the standard reduction potential for Co^(3+)(aq) + 3e^(-) rightarrow Co(s) ? Co^(3+)(aq) + e^(-) rightarrow Co^(2+)(aq) E^(@) = 1.82V Co^(2+)(aq) + 2e^(-) rightarrow Co(s) E^(@) = -0.28V

According to the standard reduction potentials: Pb^(2+)(aq) + 2e^(-) rightarrow Pb(s) E^(@) = -0.13V Fe^(2+)(aq) + 2e^(-) rightarrow Fe(s) E^(@) = -0.44 Zn^(2+)(aq) + 2e^(-) rightarrow Zn(s) E^(@) = -0.76V Which species will reduce Mn^(3+) to Mn^(2+) [E^(@) = 1.51V but will NOT reduce Cr^(3+) to Cr^(2+) [E^(@) = -0.40V]

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

Use the standard reduction potentials: Sn^(2+)(aq) + 2e^(-) rightarrow Sn(s) E^(@) = -0.141V Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.800V To calcultate E^(@) for the reaction: Sn(s) + 2Ag^(+)(aq) rightarrow Sn^(2+)(aq) + 2Ag(s)

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

According to the reductions potentials in the table below, which statements is true under standard conditions? {:("Reaction", E^(@)V), (L^(2+) + 2e^(-) rightarrow L, -0.13), (M^(2+) + 2e^(-) rightarrow M, -0.44),(N^(2+) + 2e^(-) rightarrow N, -0.76):}

For the reduction of NO_(3)^(-) ion in an aqueous solution, is +0.96V. Values of for some metal ions are given below : V^(2+)(aq)+ 2e^(-)rightarrowV , E^(@)= -1.19V Fe^(3+)(aq)+ 3e^(-) rightarrow Fe , E^(@) = -0.04 V Au^(3+)(aq) + 3e^(-) rightarrow Au , E^(@) = +1.40V Hg^(2+) (aq)+ 2e^(-) rightarrowHg , E^(@) = + 0.86 V The pair(s) of metals that is(are) oxidised by NO_(3)^(-) in aqueous solution is(are) :

Nickel metal is added to a solution containign 1.0 m Pb^(2+)(aq) and 1.0 M Cd^(2+)(aq) . Use the standard reduction potentials to determine which reaction(s) will occur. Reaction 1: Ni(s) + Pb^(2+)(aq) rightarrow Pb(s) + Ni^(2+)(aq) Reaction 2: Ni(s) + Cd^(2+)(aq) rightarrow Cd(s) + Ni^(2+)(aq) {:("Reaction", E^(@)), (Pb^(2+)(aq) + e^(-) rightarrow Pb(s) , -0.13V), (Ni^(2+)(aq) + 2e^(-) rightarrow Ni(s), -0.23V), (Cd^(2+)(aq) + 2e^(-) rightarrow Cd(s), -0.40V):}

Use the standard reduction potentials to determine what is observed at the cathode during the electrolysis of a 1.0 M solution of KBr that contains phenolphthalein. O_(2)(g) + 4H^(+)(aq) + 4e^(-) rightarrow 2H_(2)O(l) E^(@) = 1.23V Br_(2)(l) + 2e^(-) rightarrow 2Br^(-)(aq) E^(@) = 1.07V 2H_(2)O(l) + 2e^(-) rightarrow H_(2)(g) + 2OH^(-) E^(@0 = -0.80V K^(+) (aq) + e^(-) rightarrow K(s) E^(@) = -2.92V