Assume that the complete combustion of one mole of ethanol to carbon dioxide and water liberates 1370 kj of energy (δ°′=−1370 kj/mol ). if the energy generated by the combustion of ethanol is entirely converted to the synthesis of a hypothetical compound x, calculate the number of moles of the compound that could theoretically be generated. use the value δ°′compound x=−45.9 kj/mol . round your answer to two significant figures.

28 moles of X.

Explanation:

Let's consider the complete combustion of ethanol.

C₂H₆O(l) + 3 O₂(g) ⇒  2 CO₂(g) + 3 H₂O(l)

When 1 mole of ethanol burns it releases 1370 kJ, that is, the enthalpy of combustion is -1370 kJ/mol. If the energy released by one mole of etanol were used to syntesize the compound X, it would take 45.9 kJ to form 1 mole of X, that is, the enthalpy of formation is -49.5 kJ/mol. Then,

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