The preparation of NO2(g) from N2(g) and O2(g) is an endothermic reaction: N2(g) + O2(g) → NO2(g) (unbalanced).The enthalpy change of reaction for the balanced equation (with lowest whole-number coefficients) is ΔH = 67.7 kJ/mol reaction. If 291 mL of N2 and 435 mL of O2, both at 113°C and 2.65 atm, are mixed, what amount of heat is necessary to synthesize NO2?
The preparation of NO2(g) from N2(g) and O2(g) is an endothermic reaction: N2(g) + O2(g) → NO2(g) (unbalanced).The enthalpy change of reaction for the balanced equation (with lowest whole-number coefficients) is ΔH = 67.7 kJ/mol reaction. If 291 mL of N2 and 435 mL of O2, both at 113°C and 2.65 atm, are mixed, what amount of heat is necessary to synthesize NO2?
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 1RC
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The preparation of NO2(g) from N2(g) and O2(g) is an endothermic reaction: N2(g) + O2(g) → NO2(g) (unbalanced).The enthalpy change of reaction for the balanced equation (with lowest whole-number coefficients) is ΔH = 67.7 kJ/mol reaction. If 291 mL of N2 and 435 mL of O2, both at 113°C and 2.65 atm, are mixed, what amount of heat is necessary to synthesize NO2?
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