Chemistry, 09.12.2020 21:00 EricBryanLopez
A 488.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g・°C; heat capacity of liquid = 1.75 J/g・°C; ∆Hfus = 8.04 kJ/mol; Tfinal = 17.6 °C) a)How much energy (in kJ) is absorbed/released to heat the solid? b)How much energy (in kJ) is absorbed/released to melt the solid? c)How much energy (in kJ) is absorbed/released to heat the liquid? d)What is the total amount of energy that must be absorbed/released for the entire process?
Answers: 1
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A 488.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (...
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