6. Using the half reactionHCO3 +9H+ + 8e- ←⇒ CH4 (aq) + 3H₂O (1)and the fact that for a ground water, pH = 8.3 and the concentrations of HCO3-and CH4(aq) are 10-3 M and 5x10-6 M, respectively, calculate Eh and pe at 25°C.The Nernst equation for this problem is:Eh EOEº=0.0592HCO3n- AGnữ, n is number of electrons, 3=96.42 kJ volt-1 eq-¹. Assume activityequals molar concentration. Known AfG₁ = -237.1 kJ mol-1, AG = -79.4 kJH₂оCH4_=-110.8 kJ mol-¹, AƒG₁ = 0 kJ mol-1.mol-1, AfG,H+acH4ансa+-log(-

Given, aCH4=5×10-6 MaHCO3-=10-3 MaH+=10-pH=10-8.3

Using the half reaction HCO3 + 9H+ + 8e-←→ CH4 (aq) + 3H₂O (1) and the fact that for a ground water, pH = 8.3 and the concentrations of HCO3- and CH4(aq) are 10-3 M and 5x10-6 M, respectively, calculate Eh and pe at 25°C. The Nernst equation for this problem is: Eh = Eº_ Eº --AG 0.0592 HCO3 n n is number of electrons, 3-96.42 kJ volt-1 eq-¹. Assume activity equals molar concentration. Known AfG₁ = -237.1 kJ mol-1, AG = -79.4 kJ H₂O CH4 mol-¹, AfG = -110.8 kJ mol-1, AfG, = 0 kJ mol-1. H+ acH4 aHCO3 + -log(

Using the half reaction HCO3 + 9H+ + 8e-←→ CH4 (aq) + 3H₂O (1) and the fact that for a ground water, pH = 8.3 and the concentrations of HCO3- and CH4(aq) are 10-3 M and 5x10-6 M, respectively, calculate Eh and pe at 25°C. The Nernst equation for this problem is: Eh = Eº_ Eº --AG 0.0592 HCO3 n n is number of electrons, 3-96.42 kJ volt-1 eq-¹. Assume activity equals molar concentration. Known AfG₁ = -237.1 kJ mol-1, AG = -79.4 kJ H₂O CH4 mol-¹, AfG = -110.8 kJ mol-1, AfG, = 0 kJ mol-1. H+ acH4 aHCO3 + -log(

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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