Exothermic: ΔH = (-)
Endothermic: ΔH = (+)
You may want to reference (Pages 191 - 192) Section 5.8 and Appendix C (Pages 1088 - 1091) while completing this problem.
It is interesting to compare the "fuel value" of a hydrocarbon in a hypothetical world where oxygen is not the combustion agent. The enthalpy of formation of CF4(g) is -679.9 kJ/mol.
Which of the following two reactions is more exothermic?
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
CH4(g) + 4F2(g) → CF4(g) + 4HF(g)
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