From the fllowing half-cell reactions and their standard potentials ,what is the smallest possible standard e.m.f for spontaneous reactions?
`PO_4^(3-)(aq)+2H_2O(l)+2e^(-)toHPO_3^(2-)+3OH^(-)(aq), E^(@)=-1.05V`
`PbO_2(s)+H_2O(l)+2e^(-)toPbO(s)+2OH^(-)(aq),E^(@)=+0.28 V`

Consider the following half-cell reaction and associated standerd half-cell potentials and determine the maximum voltage thatr can be obtained by combination resulting in spontenous process : AuBr_(4)^(-)(aq)+3e^(-)toAu(s)+4BR^(-)(aq), E^(@)=-086V Eu^(3+)(aq)+e^(-)toEu^(2+)(aq), E^(@)=-043V Sn^(2+)(aq)+2e^(-)toSn(s), E^(@)=-0.14V IO^(-)(aq)+H_(2)O(l)+2e^(-)toI^(-)(aq)+2OH^(-), E^(@)=+0.49V

Consider the following half-cell reaction and associated standerd half-cell potentials and determine the maximum voltage thatr can be obtained by combination resulting in spontenous process : AuBr_(4)^(-)(aq)+3e^(-)toAu(s)+4BR^(-)(aq), E^(@)=-086V Eu^(3+)(aq)+e^(-)toEu^(2+)(aq), E^(@)=-043V Sn^(2+)(aq)+2e^(-)toSn(s), E^(@)=-0.14V IO^(-)(aq)+H_(2)O(l)+2e^(-)toI^(-)(aq)+2OH^(-), E^(@)=+0.49V

Consider the following half-cell reaction and associated standerd half-cell potentials and determine the maximum voltage thatr can be obtained by combination resulting in spontenous process : AuBr_(4)^(-)(aq)+3e^(-)toAu(s)+4BR^(-)(aq), E^(@)=-086V Eu^(3+)(aq)+e^(-)toEu^(2+)(aq), E^(@)=-043V Sn^(2+)(aq)+2e^(-)toSn(s), E^(@)=-0.14V IO^(-)(aq)+H_(2)O(l)+2e^(-)toI^(-)(aq)+2OH^(-), E^(@)=+0.49V

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

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potentials are given below: MnO_(4)^(-)(aq) +8H^(+)(aq) +5e^(-) rarr Mn^(2+)(aq) +4H_(2)O(l) E^(@) = 1.51V Cr_(2)O_(7)^(2-)(aq) +14H^(+) (aq) +6e^(-) rarr 2Cr^(3+)(aq) +7H_(2)O(l), E^(@) = 1.38V Fe^(3+) (aq) +e^(-) rarr Fe^(2+) (aq), E^(@) = 0.77V CI_(2)(g) +2e^(-) rarr 2CI^(-)(aq), E^(@) = 1.40V Identify the only incorrect statement regarding quantitative estimation of aqueous Fe(NO_(3))_(2)

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potentials are given below: MnO_(4)^(-)(aq) +8H^(+)(aq) +5e^(-) rarr Mn^(2+)(aq) +4H_(2)O(l) E^(@) = 1.51V Cr_(2)O_(7)^(2-)(aq) +14H^(+) (aq) +6e^(-) rarr 2Cr^(3+)(aq) +7H_(2)O(l), E^(@) = 1.38V Fe^(3+) (aq) +e^(-) rarr Fe^(2+) (aq), E^(@) = 0.77V CI_(2)(g) +2e^(-) rarr 2CI^(-)(aq), E^(@) = 1.40V Identify the only correct statement regarding quantitative estimation of aqueous Fe(NO_(3))_(2)