Calculate the standard cell potential, Ecell, for this reaction at 298 K.12 (s) +2 Br (aq) --> 21 (aq) + Br2 (aq)K 1.1 x 10-18 @ 298 KEQUATIONS AND CONSTANTSE cell= E°cell-(0.0592/n) log Q @ 25°CR = 8.314 J/mol-KAG=-nFE°cellF =9.65 x 104 J/V mol eAGTxn =-(RT)In Kcell (RT/nF) In KFor electrolysis:In (No/N) = kt1A = 1 C/st12 0.693/kF =9.65 x 10 C/mol eO- 0.89 V+ 1.09 VO + 0.22 VO-0.76 VO- 0.53 VDELLEscF1F2F3F4F5F6EZF8F9%23&

Equilibrium constant (Kc) = 1.1 × 10-18 Temperature (T) = 298 k Standard cell potential (E°) = ? •…

Calculate the standard cell potential, Ecell, for this reaction at 298 K. 12 (s) + 2 Br (aq) --> 21 (aq) + Br2 (aq) K 1.1 x 10-18 @ 298 K EQUATIONS AND CONSTANTS E cell = E°cel- (0.0592/n) log Q @ 25 °C R = 8.314 J/mol·K %3! AG rxn =-nFEcell F=9.65 x 104 J/V mol e %3D AG ren=-(RT) In K E'cell = (RT/nF) In K For electrolysis: In (No/N) = kt 1A = 1 C/s t12 0.693/k F= 9.65 x 10 C/mol e O-0.89 V + 1.09 V O + 0.22 V O-0.76 V

Calculate the standard cell potential, Ecell, for this reaction at 298 K. 12 (s) + 2 Br (aq) --> 21 (aq) + Br2 (aq) K 1.1 x 10-18 @ 298 K EQUATIONS AND CONSTANTS E cell = E°cel- (0.0592/n) log Q @ 25 °C R = 8.314 J/mol·K %3! AG rxn =-nFEcell F=9.65 x 104 J/V mol e %3D AG ren=-(RT) In K E'cell = (RT/nF) In K For electrolysis: In (No/N) = kt 1A = 1 C/s t12 0.693/k F= 9.65 x 10 C/mol e O-0.89 V + 1.09 V O + 0.22 V O-0.76 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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