(d) For the reaction: H3C. H3C, CC-OH Cc=CH2 H20 H3C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (AreactG®).

(d) For the reaction: H3C. H3C, CC-OH Cc=CH2 H20 H3C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (AreactG®).

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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the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid according to the…
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For the reaction NH,NO3(aq) –→N½0(g) + 2 H2O(1) AG° = -181.7 kJ and AH° = -149.6 kJ at 321 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 321 K. The entropy change for the reaction of 2.38 moles of NH,NO3(aq) at this temperature would be J/K.
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