A) Calculate ΔSfus of HI.
Tf = -50.91 °C + 273.15 = 222.24 K
ΔSfus = 12.9 J/mol-K
B) Calculate ΔSvap of HI.
Tb = -35.38 °C + 273.15 = 237.77 K
ΔSvap = 89.1 J/mol-K
Using the following data,
|Compound||Melting Point (C)||delta Hfus (kJ/mol)||Boiling Point (C)||delta H vap|
calculate ΔSfus and ΔSvap for HI. answers in J/(K*mol)
Determine the entropy change when 4.90 mol of HI(l) boils at atmospheric pressure. answer in (J/K)
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