Task 5.1d

Use standard electrode potentials to predict, with a reason, if the following simple redox reactions are spontaneous.
(a) Zn(s) + Cu²⁺ ---> Cu(s) + Zn²⁺(aq)
(b) Sn²⁺(aq) + I₂(aq) ---> Sn⁴⁺(aq) + 2I^-(aq)
(c) Sn⁴⁺(aq) + 2Fe²⁺(aq) ---> Sn²⁺(aq) + 2Fe³⁺(aq)
(d) 2Ce⁴⁺(aq) + 2Br^-(aq) ---> 2Ce³⁺(aq) + Br₂(l)
(e) 2Cr³⁺(aq) + 7H₂O(l) +3Cl₂ ---> Cr₂O₇^2-(aq) + 14H⁺(aq) + 6Cl^-(aq)

Zn²⁺(aq)  + 2e^- = Zn(s)  E^o = -0.76V
Cu²⁺(aq) + 2e^- = Cu(s)  E^o = +0.34V
Sn⁴⁺(aq) + 2e- = Sn²⁺(s) E^o = +0.17V
I₂(aq) + 2e^- ---> 2I^-(aq)  E^o = +0.54V
Fe³⁺(aq) + e^-   = Fe²⁺(aq) E^o = +0.77V
Ce⁴⁺(aq) + e^- ---> Ce³⁺(aq) E^o = +1.70V
Br₂(l) + 2e-    =  2Br^-(aq) E^o = +1.09V
Cr₂O₇^2- (aq)  + 14H⁺(aq) + 6e^- ---> 2Cr³⁺(aq)+ 7H₂O(l) E^o = +1.33V
Cl₂ + 2e^- --->  2Cl^-(aq)  E^o = +1.36V

Answers: (a) spontaneous, (b) spontaneous, (c) not spontaneous, (d) spontaneous, (e) spontaneous, but very close values so non-standard conditions might prevent the reaction from happening.