A 35.20 g sample of liquid antimony at 747.0 °C is poured into a mold and allowed to cool to 28.0 °C. How many kJ of energy are released in this process. Report the answer as a positive number.
boiling point = 1.440×103 °C delta16-1.GIFHvap(1.440×103 °C) = 1.605×103 J/g
melting point = 631.0 °C delta16-1.GIFHfus(631.0 °C) = 161.1 J/g
specific heat solid = 0.2090 J/g°C
specific heat liquid = 0.2590 J/g°C
Please help..I keep getting the wrong answer.
35.20g*(.2090/1)(631.0-747)= 40925.87
35.20g*(161.1/1)=5670.72
35.20g*(.2590/1)*(28.0-631.0)= -5497.4
41.09919 k/J is not the right answer...help?
