Problem: 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) + 2 O2(g) → CO2(g) + 2 H2O(g)

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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) + 2 O2(g) → CO2(g) + 2 H2O(g)

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