Question

Complete each of the following half-reactions with the correct number of electrons and then arrange them from strongest caidizing potential to strongest reducing potential Strongest Oxidizing Potential Drag the text blocks below into their correct order. Fes (aq) + + Fe (aq) = +0.77 V 2H(aq) + * H(o) +0.00 V Natal - Nais) E.-2.71 V Co (aq) + -Co" (aq) +1.82 V Br(0) + - 2Br(ad E - +1.07 v Nad) - Nis) E--0.25 V Strongest Reducting Potential

Answer 1

Fe3+(aq) + e-                      Fe2+(aq) , E0 = +0.77

2H++2e-                          H2 (g)   , E0 = +0.00

Na+(aq)+1e-                      Na(s) , E0 = -2.71

Co3+(aq)+1e-                      Co2+(aq) , E0 = +1.82

Br2(g)+2e-                       2Br-(aq)   , E0 = +1.07

Ni2++2e-                           Ni(s) , E0 = -0.25

Electrode potential refers to the tendency of the electrode to release or accept electrons. This could be oxidising or reducing potential. However, conventionally, reduction potential is referred to as electrode potential. An agent which have positive electrode potential behave as oxidising agent.

Here, Co3+ act as strong oxidising agent.

The order of oxidising potential to reducing potential are as follows,

Co3+ >Br2 >Fe3+ >H+ > Ni2+ > Na+