Question

Consider the data in the table. Compound | Melting point (°C) | ?Hfus (kJ/mol) | Boiling point (°C) | ?Hvap (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 ?Sfus and ?Svap for HCl. ?Sfus = 12.92 J/(K · mol) ?Svap = 89.05 J/(K · mol) Determine the entropy change when 3.30 mol HCl(l) freezes at atmospheric pressure. ?S = 578.82 J/K

          Consider the data in the table.

Compound | Melting point (°C) | ?Hfus (kJ/mol) | Boiling point (°C) | ?Hvap (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 ?Sfus and ?Svap for HCl.
?Sfus = 12.92 J/(K · mol)
?Svap = 89.05 J/(K · mol)

Determine the entropy change when 3.30 mol HCl(l) freezes at atmospheric pressure.
?S = 578.82 J/K

Show more…

Consider the data in the table.

Compound | Melting point (°C) | ?Hfus (kJ/mol) | Boiling point (°C) | ?Hvap (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 ?Sfus and ?Svap for HCl.
?Sfus = 12.92 J/(K · mol)
?Svap = 89.05 J/(K · mol)

Determine the entropy change when 3.30 mol HCl(l) freezes at atmospheric pressure.
?S = 578.82 J/K

Added by Paul B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

06/16/2023

Step 1

Given for HCl, \( \Delta H_{fus} = 1.991 \) kJ/mol and the melting point is -114.3°C. First, convert the melting point to Kelvin: \[ T_{m} = -114.3 + 273.15 = 158.85 \, K \] Now, plug the values into the formula: \[ \Delta S_{fus} = \frac{1.991 \, Show more…

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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 = 12.92 J/(K · mol) ΔSvap = 89.05 J/(K · mol) Determine the entropy change when 3.30 mol HCl(l) freezes at atmospheric pressure. ΔS = 578.82 J/K

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