For the following process, determine the change in entropy for the system (delta

Question

For the following process, determine the change in entropy for the system (delta S_sys), the surrounding (delta S_sys), and the universe (delta S_univ). Then identify the process as a spontaneous process, a nonspontaneous process, or an equilibrium process at the specified temperature. (Assume that the thermodynamic data will not vary with temperature.) PCl_3 (l) rightarrow PCl_3 (g) at 61.2 degree C delta H^0 _f (kJ/mol) -319.7 -288.07 S^0 (J/K middot mol) 217.1 311.7 delta S_sys = | J/K middot mol delta S_surr = J/K middot mol Delta S_univ = J/K middot mol This process is (select) because the entropy of the (select) is (select).

Explanation / Answer

deltaS reaction = entropy of PCl3(g)- entropy of PCl3(l) = 311.7-217.1= 94.6 J/mole.K

entropy change of surroundings =- enthalpy change/ (61.2+273)= (-288.07+319.7)/334.2 = -0.0946 Kj/mole.K =-94.6 J/mole.K

entropy of universe = 94.6-94.6= 0

The process is reversible because the entropy of the universe is zero.

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