Statement 1: Melting of ice at -10 ° C and 1 atm has Δ S system 0 but is non-spontaneous. Statement 2: At -10 ° C the entropy decrease of the surroundings, Δ H fus /T, exceeds the entropy increase of

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Statement 1: Melting of ice at -10 ° C and 1 atm has Δ S system >0 but is non-spontaneous. Statement 2: At -10 ° C the entropy decrease of the surroundings, Δ H fus /T, exceeds the entropy increase of the system, so Δ S total <0.

TestHub · Accepted Answer

Melting is endothermic; Δ S sys =Δ H fus /T f with T f =273 K (about 22 J/K-mol). The surroundings supply heat at 263 K: Δ S surr =-Δ H fus /263, magnitude larger than Δ H fus /273. Δ S total <0, so the process is non-spontaneous (equivalently Δ G=Δ H(1-T/T f )>0 for T<T f ). Both correct, II explains I. Answer (a).

Chemistry - Thermodynamics - II Question with Solution | TestHub

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