Consider the following reaction: 2 N2O (g) + 3 O2 (g) - > 4 NO2 (g) Standard thermodynamic values for these species at 25 oC are listed in the table below: ΔfH^o (kJ mole -1) S^o (JK-1 mole-1) NO (g) 90 211 No2 (g) 34 240 N2O (g) 82 220 O2 (g) 0 205 O3 (g) 143 239 -Calculate the standard free energy of reaction at 0 oC. - Calculate the equilibrium constant for the reaction at 0 oC.
Consider the following reaction: 2 N2O (g) + 3 O2 (g) - > 4 NO2 (g) Standard thermodynamic values for these species at 25 oC are listed in the table below: ΔfH^o (kJ mole -1) S^o (JK-1 mole-1) NO (g) 90 211 No2 (g) 34 240 N2O (g) 82 220 O2 (g) 0 205 O3 (g) 143 239 -Calculate the standard free energy of reaction at 0 oC. - Calculate the equilibrium constant for the reaction at 0 oC.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 21PS: For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data...
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Consider the following reaction: 2 N2O (g) + 3 O2 (g) - > 4 NO2 (g)
Standard
ΔfH^o (kJ mole -1) S^o (JK-1 mole-1)
NO (g) 90 211
No2 (g) 34 240
N2O (g) 82 220
O2 (g) 0 205
O3 (g) 143 239
-Calculate the standard free energy of reaction at 0 oC.
- Calculate the equilibrium constant for the reaction at 0 oC.
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