(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…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter5: Introduction To Chemical Equilibrium

Section: Chapter Questions

Problem 5.49E: 5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the...

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Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Determine the equilibrium constant for the reaction Sn+Pb2+Sn2++Pb
Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
The ionization constant, Ka, for acetic acid is 1.8 105 at 25 C. What is the value of rG for this reaction? Is this reaction product- or reactant-favored at equilibrium?
(a) The equilibrium constant of the isomerization of cis-2-butene to trans-2-butene is 2.07 at 127.0 °C. Determine the standard molar Gibbs free energy, AGR º for the reaction. (b) For C6o, the standard molar Gibbs free energy (AG, º) of formation from the elemental carbon is 23.98 kJ/mol at 25.0 °C. Determine the equilibrium constant, Keq for the formation of C60.
What is the standard enthalpy of a reaction for which the equilibrium constant is (a) doubled. (b) halved when the temperature is increased by 10 K at 298 K?

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