QUESTION 10 In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2 O2(g) → CO2(g) + 2 H₂O(l) AH = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure. 106.kJ QUESTION 11 Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: 4 NO(g) + 2 O2(g) → 4 NO2(g) ΔΗ, = ? rxn N2(g) + O2(g) → 2 NO(g) 1/2 N2(g) + O2(g) → NO2(g) Given: 117 kJ ΔΗ, = +183 kJ rxn AH rxn = +33 kJ

QUESTION 10 In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2 O2(g) → CO2(g) + 2 H₂O(l) AH = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure. 106.kJ QUESTION 11 Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: 4 NO(g) + 2 O2(g) → 4 NO2(g) ΔΗ, = ? rxn N2(g) + O2(g) → 2 NO(g) 1/2 N2(g) + O2(g) → NO2(g) Given: 117 kJ ΔΗ, = +183 kJ rxn AH rxn = +33 kJ

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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