Given: H₂O(l) $\to$ H₂O(s) $\Delta$H° = -6.02 kJ at 273K Calculate the entropy change of the surroundings ($\Delta$S_surr) when one mole of water freezes at 0 °C and a pressure of one atmosphere.

Question

Quizplus · Accepted Answer

The entropy change of the surroundings is calculated using the formula ΔS_surr = -ΔH/T. Here, ΔH = -6.02 kJ = -6020 J and T = 273 K. Thus, ΔS_surr = -(-6020 J) / 273 K = 22.1 J/K.

Given: H2O(l) →\to→ H2O(s) Δ\DeltaΔ H° = -602 KJ at 273K Calculate the Entropy Change of the 273K

Given: H₂O(l) $\to$ H₂O(s) $\Delta$ H° = -602 KJ at 273K Calculate the Entropy Change of the 273K