7. (1) Based on the information given, determine, with explanation, whether the reaction direction would favor the products or favor the reactants for each of the following cases. (a) An exothermic reaction with an increase in entropy. (b) A reaction with AG having positive sign. (2) Using a few words, explain whether using a catalyst would affect the direction of a reaction (3) For the reaction with the following energy diagram, estimate its: (a) activation, and (b) overall Gibbs Free Energy. Is this reaction exergonic or endergonic? 40 30 20 10 reaction coordinate free energy, kJ/mol

7. (1) Based on the information given, determine, with explanation, whether the reaction direction would favor the products or favor the reactants for each of the following cases. (a) An exothermic reaction with an increase in entropy. (b) A reaction with AG having positive sign. (2) Using a few words, explain whether using a catalyst would affect the direction of a reaction (3) For the reaction with the following energy diagram, estimate its: (a) activation, and (b) overall Gibbs Free Energy. Is this reaction exergonic or endergonic? 40 30 20 10 reaction coordinate free energy, kJ/mol

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 35E: Given: P4(s)+5O2(g)P4O10(s)G298=2697.0kJ/mol 2H2(g)+O2(g)2H2O(g)G298=457.18kJ/mol...

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Predicting and FULLY explain if the following reaction will be spontaneous proceed to products, or non-spontaneous, or will reach equilibrium?
How does temperature effect the following reaction in terms of its free energy?
Use the References to neces impurtant valu if needed for s atin A student determines the value of the equilibrium constant to be 1.17x10" for the following reaction. 3Fe,O3(s) + H;(g)–2Fe,0,(0) + H,O(g) Based on this value of Ke than zero. AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 2.01 moles of Fe,0,() at standard conditions at 298K. AG pan Try Another Version 1 item attempt remaining Submit Answer
(ii) Given the following information, (a) Given the data below (for 298 K) calculate the free energy of formation 4G° of H,0, in the gas phase at that temperature. (b) Calculate the value of Keg for the reaction at 298 K. AH° (kJ mol') AS° (J K' mol') H2O(g) -241.8 188.8 H2(g) 130.6 O2(g) 205.1 o o
(a) Calculate the standard free-energy change and the equilibrium constant for the dimerization of NO, to N2O4 at 25°C (see Appendix D). (b) Calculate AG for this reaction at 25°C when the pres- sures of NO2 and N,O4 are each held at 0.010 atm. Which way will the reaction tend to proceed?
Match each of the following: AH (+) and AS (+) AH (+) and AS (-) AH (-) and AS (+) AH (-) and AS (-) | Never spontaneous Spontaneous at high temperatures Always spontaneous Spontaneous at low temperatures
In the following three instances, which choice is greener ina chemical process? Explain. (a) A reaction that can be runat 350 K for 12 h without a catalyst or one that can be run at300 K for 1 h with a reusable catalyst. (b) A reagent for thereaction that can be obtained from corn husks or one thatis obtained from petroleum. (c) A process that produces noby-products or one in which the by-products are recycledfor another process.
(a) Write the chemical equation for the equilibriumthat corresponds to Kb. (b) By using the value ofKb, calculate ΔG° for the equilibrium in part (a). (c) What isthe value of ΔG at equilibrium? (d) What is the value of ΔGwhen [H+] = 6.7x 10-9 M, [CH3NH3 +] = 2.4 x 10-3 M,and [CH3NH2] = 0.098 M?
For the reaction 2Na(s) + 2H2O(1)- -2N2OH(aq) + H2(g) AH° = -368.6 kJ and AS° = -15.3 J/K The standard free energy change for the reaction of 2.11 moles of Na(s) at 276 K, 1 atm would be kJ. This reaction is (reactant, product) | | favored under standard conditions at 276 K. Assume that AH® and AS° are independent of temperature.
A student determines the value of the equilibrium constant to be 7.86x10-37 for the following reaction. H2S(g) + 2H20(1) 3H2(g) + SO2(g) Based on this value of Keg: than zero. AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 2.28 moles of H,S(g) at standard conditions at 298K. AG°rxn kJ
2. Predict whether AS is positive.or negative in each of the following processes (without doing calculations) (explain why): (a) H;0(1)H,0(g) (b) Ag"(ac) + Cl(ac)AgCl(s) (c) 4Fe(s)+302(g)2Fe;O3(s)
5) Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. (A B) cpsnc nsdo () Svods ori to lls (C avods ot to 2 HNO3(aq) + NO(g) → 3 NO2(g) + H20(1) smul K= ? AG°f (kJ/mol) -110.9 87.6 51.3 -237.1 onon ( A) 1.15 × 10-9 B) 0.980 C) 8.71 × 108 D) 1.02 E) 5.11 × 10-4 oim t gnier ng DA or oisluole (S oini aniwollol orl 00cH SI+ (9)s 8.280 0.02 e.EE (lomLD1 HA