Ti = 111.0 oC
Tf = 42.5 oC
Cg = 33.6 J/mol.oC
Lets convert mass to mol
Molar mass of H2O = 18.016 g/mol
number of mol
n= mass/molar mass
= 850.0/18.016
= 47.1803 mol
Heat released to convert vapour from 111.0 oC to 100.0 oC
Q1 = n*Cg*(Ti-Tf)
= 47.1803 mol * 33.6 J/mol.oC *(111-100) oC
= 17437.833 J
Lv = 40.67KJ/mol =
40670J/mol
Heat released to convert gas to liquid at 100.0 oC
Q2 = n*Lv
= 47.1803 mol *40670 J/mol
= 1918822.1581 J
Cl = 75.3 J/mol.oC
Heat released to convert liquid from 100.0 oC to 42.5 oC
Q3 = n*Cl*(Ti-Tf)
= 47.1803 mol * 75.3 J/mol.oC *(100-42.5) oC
= 204278.8355 J
Total heat released = Q1 + Q2 + Q3
= 17437.833 J + 1918822.1581 J + 204278.8355 J
= 2140539 J
= 2141 KJ
Since it is heat released, please enter your answer with negative sign
Answer: -2141 KJ
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