We are asked to calculate ΔH for the following reaction: CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)
Note that we need to multiply each ΔH˚ by the stoichiometric coefficient since ΔH˚ is in kJ/mol.
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
Calculate ΔH for the following reaction: CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)
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