For the reaction H₂O(l)$\rightarrow$H₂O(g) at 298 K, 1.0 atm, $\Delta$H is more positive than $\Delta$E 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 by the system in expanding against the atmospheric pressure, which is the work done in pushing back the atmosphere.

For the Reaction H2O(l) →\rightarrow→ H2O(g) at 298 K, 1 Δ\DeltaΔ H Is More Positive Than

For the Reaction H₂O(l) $\rightarrow$ H₂O(g) at 298 K, 1 $\Delta$ H Is More Positive Than