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

question 14

Multiple Choice

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

• A) 22.1 J/K
• B) -22.1 J/K
• C) 397 J/K
• D) -397 J/K
• E) 0.022 J/K

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