Asked by Kari
The standard electrode potentials for three electrode systems are:
Ti^3+(aq) + e^- --> Ti^2+ E= -0.37
Fe^3+ ---> Fe^2+(aq) E= +0.77
Ce^4(aq) + e^- ---> Ce^3+(aq) E= +1.45
Using the data above, deduce which species is the best reducing agent, giving a reason in terms of electrons for your answer.
Ti^3+(aq) + e^- --> Ti^2+ E= -0.37
Fe^3+ ---> Fe^2+(aq) E= +0.77
Ce^4(aq) + e^- ---> Ce^3+(aq) E= +1.45
Using the data above, deduce which species is the best reducing agent, giving a reason in terms of electrons for your answer.
Answers
Answered by
DrBob222
I remember that oxidation is the loss of electrons so the easiest to lose electrons will be the best reducing agent. Or the most reluctant to add electrons will be the best reducing agent. Wouldn't that be Ti? Check my thinking.
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