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Using the technique of the previous problem ΔE was found to be -2,000.00 kJ/mol of an...

Using the technique of the previous problem ΔE was found to be -2,000.00 kJ/mol of an unknown liquid hydrocarbon at 298 K. In another experiment, it was determined that for each mole of hydrocarbon, 5 moles of oxygen gas is consumed and 9 moles of CO2 gas and 4 moles of H2O liquid are produced. Find ΔH per mole of this hydrocarbon (in kJ) at 298 K.

Hint given in feedback.

Not used to answer the question: This question is a bit awkward and unrealistic for molar amounts, but allows for random numbers.

An example of a possible reaction is: C2H4(OH)2(l) +2.5O2(g) →2CO2(g)+ 3H2O(l)

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