What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 5.29 × 10-4 Mand the Cr³+ concentration is 1.41 M?3Ag+ (aq) + Cr(s) → 3Ag(s) + Cr³+ (aq)Ag+ (aq) + e¯ → Ag(s) EredCr³+ (aq) + 3e¯ → Cr(s) Eered0.799 V= -0.740 VV=EcellThe cell reaction as written above is spontaneous for the concentrations given:truefalse For the reactionN₂ (g) + 2O2(g) → 2NO2(g)- 122 J/KAH° = 66.4 kJ and AS=The equilibrium constant for this reaction at 343.0 K isAssume that AH° and AS are independent of temperature.

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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 5.29 × 10-4 M and the Cr³+ concentration is 1.41 M? 3Ag+ (aq) + Cr(s) → 3Ag(s) + Cr³+ (aq) Ag+ (aq) + e → Ag(s) Fo = 0.799 V red Cr³+ (aq) + 3e → Cr(s) E = -0.740 V red Ecell = The cell reaction as written above is spontaneous for the concentrations given: O true O false V

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 5.29 × 10-4 M and the Cr³+ concentration is 1.41 M? 3Ag+ (aq) + Cr(s) → 3Ag(s) + Cr³+ (aq) Ag+ (aq) + e → Ag(s) Fo = 0.799 V red Cr³+ (aq) + 3e → Cr(s) E = -0.740 V red Ecell = The cell reaction as written above is spontaneous for the concentrations given: O true O false V

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 15P

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