Chemistry, 29.11.2020 21:30 Snowball080717
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; ∆Hfusion = 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: 2
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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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