Using the standard free energies of formation:BaCO3(s), AG° = -1139.0 kJ mol-!BaSO4(s), AGº = -1353.0 kJ mol-CO2(g), AG° = -394.4 kJ mol·'SO3(g), AG, = -370.0 kJ mol·!calculate the standard free energy change, AG', for the reaction:BaCO3(s) + S03(g) → BaSO4(s) + CO2(g)(a)(d) 1727.6 kJ189.6 kJ(b) -238.4 kJ(c)-472.4 kJ(e)not listed here

The given data : ∆Gf°(BaCO3,s) = -1139.0 kJ/mol ∆Gf°(BaSO4,s) = -1353.0 kJ/mol ∆Gf°(CO2 ,g) = -394.4…

Using the standard free energies of formation: BaCO3(s), AG° = -1139.0 kJ mol-! BaSO4(s), AG, = -1353.0 kJ mol- CO2(g), AG° = -394.4 kJ mol-" SO3(g), AG° = -370.0 kJ mol-' alculate the standard free energy change, AG°, for the reaction: BaCO3(s) + SO3(g) → BaSO4(s) + CO2(g)

Using the standard free energies of formation: BaCO3(s), AG° = -1139.0 kJ mol-! BaSO4(s), AG, = -1353.0 kJ mol- CO2(g), AG° = -394.4 kJ mol-" SO3(g), AG° = -370.0 kJ mol-' alculate the standard free energy change, AG°, for the reaction: BaCO3(s) + SO3(g) → BaSO4(s) + CO2(g)

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...

See similar textbooks

Similar questions

4. The standard free energy (AG°) for a reaction at 298 K is -104 J / mol. What is Keq for this reaction?
a) For a reaction with AH = -152.6 kJ mol-¹ and AS°= -543.8 J K-¹ mol-¹ at 25 °C, how will AGº change if the reaction temperature is increased? Explain your answer. b) Calculate the equilibrium constant for the reaction at 80 °C, showing your working (assume AH and AS° are temperature independent).
[Review Topics] [References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.21x1012 for the following reaction. CO(g) + Cl2(g)- COC12(g) Based on this value of Keg AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.65 moles of CO(g) at standard conditions at 298K. AG rxn kJ
Calculate standard free energy change using AGf values. Consider the reaction 2NH3(g) + 3N₂O(g)4N₂(g) + 3H₂O(g) Use standard free energies of formation to calculate the standard free energy change for this reaction at 25°C. kJ/mol AG° = rxn
A student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K. G°rxn = ____kJ
What is the standard free energy change for the ionization of H2O2 acid, if its Ka is 2.40e-12. 66.326 kJ -66.326 kJ -152.749 kJ 152.749 kJ
24
For the reaction CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) ΔΗ° - 206.1 kJ and AS = - 214.7 J/K The standard free energy change for the reaction of 1.67 moles of CO(g) at 253 K, 1 atm would be This reaction is favored under standard conditions at 253 K. Assume that AH° and AS° are independent of temperature. == kJ.
What’s the answer for this
Calculate The Equilibrium Constant K of hydrosulfuric acid (H2S(aq)) Standard Gibbs Free energy for H2S(aq) is -27.7Then, Calculate the pKa1 and pKa2 of hydrosulfuric acid
A student determines the value of the equilibrium constant to be 8.18x10-37 for the following reaction. H₂S(g) + 2H₂O(l)—3H₂(g) + SO₂(g) Based on this value of Keq: AG° for this reaction is expected to be (greater, less) zero. than Calculate the free energy change for the reaction of 1.68 moles of H₂S(g) at standard conditions at 298K. AG rxn= kJ
A student determines the value of the equilibrium constant to be 1.87x107 for the following reaction. Fe(s) + 2HCI(aq)- →FECI2(s) + H2(g) Based on this value of Keg: AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.39 moles of Fe(s) at standard conditions at 298K. kJ rxn