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If the temperature of the surroundings is 38.36 °C, calculate the entropy change (in J/K) for...

If the temperature of the surroundings is 38.36 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 48.1 g of gaseous carbon tetrachloride (CCl4) condenses. Report your answers to two decimal places.

Tfus(°C) -23.00

Tvap(°C) 76.80

ΔH°fus (kJ/mol) 3.28

ΔH°vap (kJ/mol) 29.82

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Homework Answers

Answer #1

During condesnation Gaseous Carbon tetrachloride looses latent heat of vaporization. Hence

Molecular weoght of CCl4= 154 g/mole, moles of CCl4 in 48.1 gm = 48.1/154=0.3123 moles

Heat lost by CCl4 during condensation= 29.82Kj/mole*0.3123=9.312 Kj =9132 joules

Entropy change of system = -9132/ (76.8+273.15)= -26.09 j/K

This heat has to be transfered to the surroundings in adiabatic system

Hence entropy change of surroudings = 9132/ (38.36+273.15) j/K=29.32 j/K

entroypy change of universe= entropy change of system + entropy change of surrounigs= 29.32- 26.09=3.23 j/K

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