A 127.7 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0...

 

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A 127.7 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 C to 147.6 C. (heat capacity of liquid = 1.62 J/g. C; heat capacity of gas = 1.04 J/g- C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 C) L How much energy (in kJ) is absorbed/released to cool the gas? How much energy (in kJ) is absorbed/released to condense the gas? How much energy (in kJ) is absorbed/released to cool the liquid? What is the total amount of energy that must be absorbed/released for the entire process? > 0/1 Point Earned 3/3 Attempts Remaining 0/1 Point Earned 3/3 Attempts Remaining 0/1 Point Earned 3/3 Attempts Remaining 0/1 Point Earned. 3/3 Attempts Remaining A 127.7 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 C to 147.6 C. (heat capacity of liquid = 1.62 J/g. C; heat capacity of gas = 1.04 J/g- C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 C) L How much energy (in kJ) is absorbed/released to cool the gas? How much energy (in kJ) is absorbed/released to condense the gas? How much energy (in kJ) is absorbed/released to cool the liquid? What is the total amount of energy that must be absorbed/released for the entire process? > 0/1 Point Earned 3/3 Attempts Remaining 0/1 Point Earned 3/3 Attempts Remaining 0/1 Point Earned 3/3 Attempts Remaining 0/1 Point Earned. 3/3 Attempts Remaining

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To answer these questions we need to use the thermodynamic properties provided for the unknown substance and apply some basic calorimetry equations Ac... View the full answer