Ti = 121.0 oC
Tf = 19.0 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
= 1250.0/18.016
= 69.3828 mol
Heat released to convert vapour from 121.0 oC to 100.0 oC
Q1 = n*Cg*(Ti-Tf)
= 69.3828 mol * 33.6 J/mol.oC *(121-100) oC
= 48956.4831 J
Lv = 40.67KJ/mol =
40670J/mol
Heat released to convert gas to liquid at 100.0 oC
Q2 = n*Lv
= 69.3828 mol *40670 J/mol
= 2821797.2913 J
Cl = 75.3 J/mol.oC
Heat released to convert liquid from 100.0 oC to 19.0 oC
Q3 = n*Cl*(Ti-Tf)
= 69.3828 mol * 75.3 J/mol.oC *(100-19) oC
= 423186.3344 J
Total heat released = Q1 + Q2 + Q3
= 48956.4831 J + 2821797.2913 J + 423186.3344 J
= 3293940 J
= 3294 KJ
Since it is heat released, please enter your answer with negative sign
Answer: -3294 KJ
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