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10 Nov 2019
Using the standard reduction potentials given in Appendix of your text book, calculate the cell potential (E*_cell) at 298 K for each of the following reactions. (A) Br_2 (aq) + 2 Cl^- (aq) rightarrow 2Br^- (aq) + Cl_2 (g) -0.27 V (B) Au^3+ (aq) + 3Ag (s) rightarrow Au (s) + 3Ag^+ (aq) +0.70 V (C) A Galvanic Cell with the SHE and Cr^3+/Cr(s) +0.73 V For the reactions listed in Question 3, calculate the Standard free energy change Delta G degree at 298 K. Indicate whether the reactions are spontaneous or not. A) +52.1 kJ Nonspontaneous (B) -203 kJ Spontaneous C) -423 kJ Spontaneous
Using the standard reduction potentials given in Appendix of your text book, calculate the cell potential (E*_cell) at 298 K for each of the following reactions. (A) Br_2 (aq) + 2 Cl^- (aq) rightarrow 2Br^- (aq) + Cl_2 (g) -0.27 V (B) Au^3+ (aq) + 3Ag (s) rightarrow Au (s) + 3Ag^+ (aq) +0.70 V (C) A Galvanic Cell with the SHE and Cr^3+/Cr(s) +0.73 V For the reactions listed in Question 3, calculate the Standard free energy change Delta G degree at 298 K. Indicate whether the reactions are spontaneous or not. A) +52.1 kJ Nonspontaneous (B) -203 kJ Spontaneous C) -423 kJ Spontaneous
Jean KeelingLv2
7 Aug 2019