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At 298 K, the standard reduction potenti...

At 298 K, the standard reduction potentials are 1.51 V for `MnO_(4)^(-) | Mn^(2+), 1.36 V` for `Cl^(2) | Cl^(-)`, 1.07 V for `Br_(2)|Br^(-),` and 0.54 V for `I_(2)|I^(-)`. At pH=3, permanganate is expected to oxidize `((RT)/(F) = 0.059V)`:

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At 298 K, the standard reduction potentials are 1.51 V for MnO_(4)^(-), Mn^(2+),1.36V for Cl_(2)/CI^(-) , 1.07 V Br_(2)|. Br^(-) , and 0.54 V for l_(2)|l^(-) At pH=3, permaganate is expected to oxidize (2.303RT/F -0.059 V)

At 298 K, the standard reduction potential are: 1.33 V for Cr_(2)O_(7)^(2-) | Cr^(3+) , 1.36 V for Br_(2)|Br^(-) and 0.54V for I_(2)|I^(-) . At pH = 4, Cr_(2)O_(7)^(2-) is expected to oxidise? Assume [Cr^(3+)] = [Cr_(2)O_(7)^(2-)] = 1M.

Find the standard electrode potential of MnO_(4)^(c-)|MnO_(2). The standard electrode potential of MnO_(4)^(c-)|Mn^(2+)=1.51V and MnO_(2)|MnO_(2)|Mn^(2+)=1.23V .

Find the standard electrode potential of MnO_(4)^(c-)|MnO_(2). The standard electrode potential of MnO_(4)^(c-)|Mn^(2+)=1.51V and MnO_(2)|MnO_(2)|Mn^(2+)=1.23V .

Find the standard electrode potential of MnO_(4)^(c-)|MnO_(2). The standard electrode potential of MnO_(4)^(c-)|Mn^(2+)=1.51V and MnO_(2)|MnO_(2)|Mn^(2+)=1.23V .

Find the standard electrode potential of MnO_(4)^(c-)|MnO_(2). The standard electrode potential of MnO_(4)^(c-)|Mn^(2+)=1.51V and MnO_(2)|MnO_(2)|Mn^(2+)=1.23V .

The reduction potentials are : Cl_2+2e^(-)=2Cl^(-) " "E^@=1.36V F_2+2e^(-) =2F^(-) " "E^@=2.87 V Which is a better oxidising agent?