Problem: Using the following data, Compound     Melting point (°C)     ΔHfus (kJ/mol)     Boiling point (°C)     ΔHvap (kJ/mol)HF                   -83.11                         4.577                   19.54                        25.18HCl                 -114.3                          1.991                   -84.9                         17.53HBr                 -86.96                       2.406                  -67.0                         19.27Hl                    -50.91                        2.871                   -35.38                       21.16calculate ΔSfus and ΔSvap for HCl. Determine the entropy change when 6.00 mol of HCl(s) melts at atmospheric pressure.

FREE Expert Solution

Step 1: ΔSvap 


∆Svap = ∆HvapTb


T = -84.9°C + 273.15 = 188.25 K

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Problem Details

Using the following data, 

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

Hl                    -50.91                        2.871                   -35.38                       21.16

calculate ΔSfus and ΔSvap for HCl. 

Determine the entropy change when 6.00 mol of HCl(s) melts at atmospheric pressure.

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