5. The chemistry of nitrogen oxides is very versatile. Given the following reactions and their standard enthalpy changes, AHxn AHO AHxn = -57.2 kJ /mol AHxn = -114.2 kJ /mol AHxn = -54.1 kJ/mol -39.8 kJ/mol = -112.5 kJ /mol (1) NO(g) + N02 (g) → N203(g) (2) NO(g) + NO2(g) + 02(g) → N205(g) (3) 2 NO2(g) → N2O4(g) (4) 2 NO(g) + 02(g) → 2 NO2(g) (5) N205(s) → N½05(g) rxn calculate the standard enthalpy of reaction (with complete solution, include the reactions) for N203(g) + N205 (s) → 2 N204(g)
5. The chemistry of nitrogen oxides is very versatile. Given the following reactions and their standard enthalpy changes, AHxn AHO AHxn = -57.2 kJ /mol AHxn = -114.2 kJ /mol AHxn = -54.1 kJ/mol -39.8 kJ/mol = -112.5 kJ /mol (1) NO(g) + N02 (g) → N203(g) (2) NO(g) + NO2(g) + 02(g) → N205(g) (3) 2 NO2(g) → N2O4(g) (4) 2 NO(g) + 02(g) → 2 NO2(g) (5) N205(s) → N½05(g) rxn calculate the standard enthalpy of reaction (with complete solution, include the reactions) for N203(g) + N205 (s) → 2 N204(g)
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
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.7: Enthalpy Calculations
Problem 2RC
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