Given the following information, use Hess’s law to calculate ΔH for the reaction: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g) 4C(s) + 5H2(g) → C4H10(g) ΔH = –126 kJC(s) + O2(g) → CO2(g) ΔH = –393.5 kJH2(g) + ½ O2(g) → H2O(g) ΔH = –241.8 kJ -509 kJ -5818 kJ -5314 kJ -761.8 kJ
Given the following information, use Hess’s law to calculate ΔH for the reaction: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g) 4C(s) + 5H2(g) → C4H10(g) ΔH = –126 kJC(s) + O2(g) → CO2(g) ΔH = –393.5 kJH2(g) + ½ O2(g) → H2O(g) ΔH = –241.8 kJ -509 kJ -5818 kJ -5314 kJ -761.8 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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Given the following information, use Hess’s law to calculate ΔH for the reaction:
2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
4C(s) + 5H2(g) → C4H10(g) ΔH = –126 kJ
C(s) + O2(g) → CO2(g) ΔH = –393.5 kJ
H2(g) + ½ O2(g) → H2O(g) ΔH = –241.8 kJ
-509 kJ
-5818 kJ
-5314 kJ
-761.8 kJ
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