For the reaction H₂O(l)$\to$ H₂O(g)at 298 K and 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 in energy is due to the work required to expand the gas against atmospheric pressure when the substance changes from liquid to gas, which is the work done in pushing back the atmosphere.

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

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