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b) Using the thermodynamic data below, find the numerical value for K at T = 25.0 °C. AH (kJ/mole) AG (kJ/mole) S (J/mole K) Substance (50₂)² (PO₂) O₂(g) -SO₂(g) SO3(s) 0.0 296.4 395.2 0.0 300.4 370.4 205.0 248.5 256.2

b) Using the thermodynamic data below, find the numerical value for K at T = 25.0 °C. AH (kJ/mole) AG (kJ/mole) S (J/mole K) Substance (50₂)² (PO₂) O₂(g) -SO₂(g) SO3(s) 0.0 296.4 395.2 0.0 300.4 370.4 205.0 248.5 256.2

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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CHM 1046 - JOENS WORKSHEET #7 Due date: Wednesday, October 11 NAME Katherine Bustillo Panther ID 6359232 For problems involving calculations you must show your work for credit. 1) Sulfur dioxide (SO₂) can react with molecular oxygen (O₂) to form sulfur trioxide (SO3) by the process 2 SO:(g) + O₂(g) 2 SO(g) a) Give the correct expression for K, the thermodynamic equilibrium constant, for the above (PSO3)2 (50₂) ² (₂) reaction. K b) Using the thermodynamic data below, find the numerical value for K at T = 25.0 °C. Substance AH° (kJ/mole) AG (kJ/mole) S°(J/mole K) O₂(g) SO₂(g) SO3(s) 0.0 - 296.4 - 395.2 0.0 - 300.4 370.4 205.0 248.5 256.2
Transcribed Image Text:CHM 1046 - JOENS WORKSHEET #7 Due date: Wednesday, October 11 NAME Katherine Bustillo Panther ID 6359232 For problems involving calculations you must show your work for credit. 1) Sulfur dioxide (SO₂) can react with molecular oxygen (O₂) to form sulfur trioxide (SO3) by the process 2 SO:(g) + O₂(g) 2 SO(g) a) Give the correct expression for K, the thermodynamic equilibrium constant, for the above (PSO3)2 (50₂) ² (₂) reaction. K b) Using the thermodynamic data below, find the numerical value for K at T = 25.0 °C. Substance AH° (kJ/mole) AG (kJ/mole) S°(J/mole K) O₂(g) SO₂(g) SO3(s) 0.0 - 296.4 - 395.2 0.0 - 300.4 370.4 205.0 248.5 256.2
Expert Solution
Step 1: Relationship between equilibrium constant,k & standard Gibbs free energy change ∆G° :

Relationship between equilibrium constant,k & standard Gibbs free energy change ∆G° is 

∆G° = - RTln K

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