Compound
Melting point (°C)
ΔHfus (kJ/mol)
Boiling point (°C)
ΔHvap (kJ/mol)
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
HI
-50.91
2.871
-35.38
21.16
Using the data in the table, calculate
ΔSfus and
ΔSvap for HCl.
ΔSfus = J/(K⋅mol)
ΔSvap = J/(K⋅mol)
Determine the entropy change when 6.90 mol
of HCl(l) freezes at atmospheric pressure.
ΔS = J/K