For the reaction NO(g) + NO₂(g) the following questions. Substance NO(g) NO₂(g) N₂O(g) N₂O3 (9) N₂O4 (9) N₂O5 (9) N₂O5 (8) AHºt So (kJ.mol-¹) (J.mol-¹.K-¹) 90.25 210.7 33.2 kJ 82.05 83.72 9.16 11 N₂O3(g), use thermodynamic data from the following table to calculate AH and AS°. Then use those values to answer -43.1 240.0 219.7 321.28 304.2 356 178 (a) Is this reaction spontaneous at 25°C? Explain your answer. The calculated AH and AS values result in a AG (in kJ) of (b) How will the spontaneity of the reaction change as the temperature increases? As the temperature increases, the TAS term of the Gibbs free energy equation will become more indicating a reaction. (c) To show that your prediction is accurate, calculate AG (in kJ) at 71°C. (Assume that both enthalpy and entropy are independent of temperature.) kJ at 25° C. Since AG is this reaction is and the value for AG
For the reaction NO(g) + NO₂(g) the following questions. Substance NO(g) NO₂(g) N₂O(g) N₂O3 (9) N₂O4 (9) N₂O5 (9) N₂O5 (8) AHºt So (kJ.mol-¹) (J.mol-¹.K-¹) 90.25 210.7 33.2 kJ 82.05 83.72 9.16 11 N₂O3(g), use thermodynamic data from the following table to calculate AH and AS°. Then use those values to answer -43.1 240.0 219.7 321.28 304.2 356 178 (a) Is this reaction spontaneous at 25°C? Explain your answer. The calculated AH and AS values result in a AG (in kJ) of (b) How will the spontaneity of the reaction change as the temperature increases? As the temperature increases, the TAS term of the Gibbs free energy equation will become more indicating a reaction. (c) To show that your prediction is accurate, calculate AG (in kJ) at 71°C. (Assume that both enthalpy and entropy are independent of temperature.) kJ at 25° C. Since AG is this reaction is and the value for AG
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.50PAE: For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then...
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Step 1: Enthalpy, entropy, and Gibbs free energy
VIEWStep 2: Determination of enthalpy of the reaction
VIEWStep 3: Determination of entropy of the reaction
VIEWStep 4: Gibbs free energy at 25oC
VIEWStep 5: Effect of increase in temperature on Gibbs free energy
VIEWStep 6: Gibbs free energy at 71oC
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