CHM 116 Homework #16 Due August 1, 2017 1. Calculate ΔGand K for the following electrochemical...
CHM 116 Homework #16 Due August 1, 2017
1. Calculate ΔGand K for the following electrochemical cell (Sample Exercise 17.7) (5 pts):
Pt|Sn2+ (1M),Sn4+ (1M)||NO3 (1M),H+ (1M),NO(1atm)|Pt
2. Calculate ΔGand Eo for the following electrochemical cell at
98.0oC (Sample Exercise 17.7)
(5 pts):
Cu|Cu2+ (1M),||Zn2+ (1M)|Zn
3. Calculate E cell for the following electrochemical cell
(Sample Exercise 17.6) (3 pts):
Pt | Fe 2+ (0.0725 M), Fe3+ (0.110 M) | | MnO4 (0.0822 M), H+
(1.00 M), Mn2+ (0.0205 M) | Pt
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CHM 116 Homework #16 Due August 1, 2017
1. Calculate ΔGand K for the following electrochemical...
Calculate Ecell (the reduction potential for the balanced chemical equation under nonstandard conditions) for the electrochemical...
Calculate Ecell (the reduction potential for the balanced chemical equation under nonstandard conditions) for the electrochemical cell shown below: Pt | Fe2+ (4.25x10-3 M), Fe3+ (1.50x10-3 M) || MnO4 - (6.50x10-3 M), Mn2+ (2.00x10-2 M), H+ (0.100 M) | Pt. Use the following standard reduction potentials for each half reaction. The Eo for Fe3+/Fe2+ = 0.77 V and Eo for MnO4 - /Mn2+ = 1.51 V.
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2...
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2 ] = 0.774 M and [Sn2 ] = 0.0190 M. Standard reduction potentials can be found here. Reduction Half-Reaction Standard Potential Ered° (V) F2(g) + 2e– → 2F–(aq) +2.87 O3(g) + 2H3O+(aq) + 2e– → O2(g) + 3H2O(l) +2.076 Co3+(aq) + e– → Co2+(aq) +1.92 H2O2(aq) + 2H3O+(aq) + 2e– → 2H2O(l) +1.776 N2O(g) + 2H3O+(aq) + 2e– → N2(g) + 3H2O(l) +1.766 Ce4+(aq) + e– → Ce3+(aq)...
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