→ N203(g)AH°(1) NO(g) + NO2(g)=-39.8 kJrxn→ N2O5(g)AH°rxn(2) NO(g) + NO2(g) + O2(g)=-112.5 kJ(3) 2NO2(g) → N2O4(g)AH:-57.2 kJrxn(4) 2NO(g) + 02g)→ 2NO2(g)AH°=-114.2 kJrxnAH°subl(5) N2O5(s)N2O5(g)= 54.1 kJCalculate the heat of reaction forN203(g) + N2O5(s) → 2N2O4(g)ΔΗ-kJ

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he heat of reaction f

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

→ N203(g)
AH°
(1) NO(g) + NO2(g)
=-39.8 kJ
rxn
→ N2O5(g)
AH°
rxn
(2) NO(g) + NO2(g) + O2(g)
=-112.5 kJ
(3) 2NO2(g) → N2O4(g)
AH
:-57.2 kJ
rxn
(4) 2NO(g) + 02g)
→ 2NO2(g)
AH°
=-114.2 kJ
rxn
AH°
subl
(5) N2O5(s)
N2O5(g)
= 54.1 kJ
Calculate the heat of reaction for
N203(g) + N2O5(s) → 2N2O4(g)
ΔΗ-
kJ

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