Given: H₂O(l)$\to$ H₂O(g) $\Delta$H° = 40.7 kJ at 373K What is the entropy change in the system ($\Delta$S) when one mole of water vaporizes at 100 °C and a pressure of one atmosphere?

Question

Quizplus · Accepted Answer

The given equation represents the enthalpy change for the vaporization of one mole of water at 373 K. However, we need to find the entropy change. We can use the following equation:
ΔS = ΔH/T
where ΔS is the entropy change, ΔH is the enthalpy change, and T is the temperature in Kelvin.

Substituting the values, we get:
ΔS = 40.7 kJ/mol / 373 K
ΔS = 109 J/K

Note that the sign does not matter for this question as we are only asked for the magnitude of the entropy change.

Given: H2O(l) →\to→ H2O(g) Δ\DeltaΔ H° = 407 KJ at 373K What Is the Entropy Change in 373K

Given: H₂O(l) $\to$ H₂O(g) $\Delta$ H° = 407 KJ at 373K What Is the Entropy Change in 373K