Use the standard half-cell potentials listed below to calculate the standard cel

Question

Use the standard half-cell potentials listed below to calculate the standard cell potential for the r following reaction occurring in an electrochemical cell at 25 degree C. (The equation is balanced.) 3 Cl^2(g) + 2 Fe(s) - 6 Cl^1(aq) + 2 Fe^3+(aq) Cl_2(g) + 2 e- rightarrow 2 Cl^-(aq) E degree = +1.36 V Fe^3+(aq) + 3 e- rightarrow Fe(s) E degree = -0.04 V +4.16 V +1.40 V +1.32 V -1.40 V -1.32 V Based on the following information, Br_2(l) + 2 e- = 2 Br^-(aq) E degree = +1.09 V Mg^2+(aq) + 2e^- rightarrow 2 Mg(s) E degree = -2.37 V which of the following chemical species is the strongest reducing agent? Mg^2+(aq) Br^-(aq) Br^2(l) Mg(s)

Explanation / Answer

3Cl2(g) + 2Fe(s)------------> 6Cl- (aq) + 2Fe3+

      Fe(s) -------------> Fe+3 (aq) + 3e-      E0 = 0.04V

   Cl2(g) +2e- --------> 2Cl- (aq)             E0 = 1.36V

   2Fe(s) -------------> 2Fe+3 (aq) + 6e-      E0 = 0.04V

   3Cl2(g) +6e- --------> 6Cl- (aq)             E0 = 1.36V

------------------------------------------------------------------------

3Cl2(g) + 2Fe(s)------------> 6Cl- (aq) + 2Fe3+ (aq) Ecell = 1.40V

B) 1.40V

Br2(l) + 2e- ------> 2Br- (aq)      E0 = 1.09V

Mg+2 (aq) + 2e- ------>2 Mg(s) E0 = -2.37V

Negative reduction potential ions arestrong reducing agent.

A) Mg+2 (aq)

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