Problem: Using the following data, Compound  Melting Point (C)  delta Hfus (kJ/mol)  Boiling Point (C)  delta H vap  HF -83.11 4.577 19.54 25.18 HCl -114.3 1.991 -84.9 17.53 HBr -86.96 2.406 -67.0 19.27 Hl -50.91 2.871 -35.38 21.16calculate 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)

FREE Expert Solution

A) Calculate ΔSfus of HI.

Tf = -50.91 °C + 273.15  = 222.24 K 


ΔSfus = ΔHfus TfΔSfus = 2.871 kJ/mol222.24 KΔSfus = 0.0129 kJmol-K ×103 J1 kJ

ΔSfus  = 12.9 J/mol-K


B) Calculate ΔSvap of HI.

Tb = -35.38 °C + 273.15  = 237.77 K 


ΔSvap = ΔHvap TbΔSvap = 21.16 kJ/mol237.77 KΔSvap = 0.0891 kJmol-K ×103 J1 kJ

ΔSvap  = 89.1 J/mol-K


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Problem Details

Using the following data,

 Compound  Melting Point (C)  delta Hfus (kJ/mol)  Boiling Point (C)  delta H vap 
 HF -83.11 4.577 19.54 25.18
 HCl -114.3 1.991 -84.9 17.53
 HBr -86.96 2.406 -67.0 19.27
 Hl -50.91 2.871 -35.38 21.16

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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