In a vacuum bottle, 320 g of water and 120 g of ice are initially in equilibrium at 0.00∘∘c. the bottle is not a perfect insulator. over time, its contents come to thermal equilibrium with the outside air at 25.0∘∘c. 1) how much does the entropy of universe increase in the process?

Δ

Explanation:

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To find the change in the entropy of the universe, we must take into account the following entropy balance:

Δ

We can stand the universe as the surroundings so the equals the outside air temperature. Then, we must compute both the water's and ice's released heat due to their interaction with the "hot" air:

Finally, we obtain the change (increasing) in the entropy of the universe as follows:

Δ

Δ

* All the data were extracted from Cengel's thermodynamics book.

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"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"

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