Homework Answers
Ti = 717.0 oC
Tf = 23.0 oC
Cl = 1.339 J/g.oC
Heat released to convert liquid from 717.0 oC to 649.0 oC
Q1 = m*Cl*(Ti-Tf)
= 20.4 g * 1.339 J/g.oC *(717-649) oC
= 1857.4608 J
Hf = 368.3 J/g
Heat released to convert liquid to solid at 649.0 oC
Q2 = m*Hf
= 20.4g *368.3 J/g
= 7513.32 J
Cs = 1.017 J/g.oC
Heat released to convert solid from 649.0 oC to 23.0 oC
Q3 = m*Cs*(Ti-Tf)
= 20.4 g * 1.017 J/g.oC *(649-23) oC
= 12987.4968 J
Total heat released = Q1 + Q2 + Q3
= 1857.4608 J + 7513.32 J + 12987.4968 J
= 22358 J
= 22.36 KJ
Answer: 22.36 KJ
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The following information is given for magnesium at 1 atm: AHvap (1090.00°C) = 5.424 x 109 J/g AH fus (649.00°C) = 368.3 J/g To = 1090.00°C Tm = 649.00°C Specific heat solid = 1.017 J/g °C Specific heat liquid = 1.339 J/g °C A 35.30 g sample of liquid magnesium at 703.00°C is poured into a mold and allowed to cool to 23.00°C. How many kJ of energy are released in this process? (Report the...
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