(b)Consider the dissociation of molecular chlorine, with an equilibrium constant K =0.44, at a certain temperature and a pressure of 1.00 bar, described by thefollowing chemical equilibrium reaction:Cl2(g) = 2 Cl(g),Calculate the following:(i) The dissociation temperature (in Kelvins) of molecular chlorine, given that thestandard Gibbs free energy change of the reaction is AG = 19 kJ mol-1.(ii) The degree of dissociation (a) of molecular chlorine(iii) If the equilibrium constant at a higher temperature of 3455 K is K = 3.00, calculateAH, assuming A.He to be constant up to this temperature range.(iv) Calculate A-GⓇ and A.SⓇ at a temperature of 3455 K.(v) Describe the position of equilibrium based on question (iv) above on the value ofAGº.

Part - I :- Dissociation temperature Given, K = 0.44 & ΔG°=19kJ/mol (19000J/mol)By using…

Answered: (b) Consider the dissociation of…

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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At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4B(g) 2 C(g) + 3D(g) were found to be PA = 4.71 atm, PB = 4.26 atm, Pc = 5.75 atm, and P = 4.58 atm. What is the standard change in Gibbs free energy of this reaction at 25 °C? AGrxn = kJ mol
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