Determine the voltage (V) of the following cell at 25°C: Zn(s) | Zn2+(aq, 0.37 M) || Cl-laq, 0.75 M) C12(g, 0.750 atm)| Pt Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e –> 2C1-(aq); E° = +1.36 V Hg2Cl2(s) + 2e –> 2Hg(l) + 2Cl(aq); E° = +0.27 V AgCl(s) + e –> Ag(s) + Cl (aq); E° = +0.22 V Ni2+(aq) + 2e –> Ni(s); E° = -0.23 V Co2+ (aq) + 2e –> Co(s); E° = -0.28 V Zn2+ (aq) + 2e –> Zn(s); E° = -0.76 V 2H2O(1) + 2e –> H2(g) + 2OH-(aq); E° = -0.83 V Your Answer: Your Answer