For the reaction H₂O(l) → H₂O(g) at 298 K, 1.0 atm, ΔH is more positive than ΔE by 2.5 kJ/mol. This quantity of energy can be considered to be

Question

Quizplus · Accepted Answer

The difference between ΔH and ΔE is due to the work done in pushing back the atmosphere as the substance goes from liquid to gas. Therefore, choice B is the correct answer. Choice A is not correct because it refers to a different thermodynamic quantity (heat flow), and choice C is not correct because it refers to the value of ΔH itself, not the difference between ΔH and ΔE. Choice D is not correct because it refers to a specific bond energy, which may not be the cause of the difference between ΔH and ΔE. Finally, choice E is not correct because there is a clear best choice, which is B.

For the Reaction H2O(l) → H2O(g) at 298 K, 1

For the Reaction H₂O(l) → H₂O(g) at 298 K, 1