Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

13. Liquids, Solids & Intermolecular Forces

Clausius-Clapeyron Equation

General Chemistry

13. Liquids, Solids & Intermolecular Forces

Clausius-Clapeyron Equation

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Multiple Choice

The vapor pressure of SiCl4 is 100 mmHg at 5.4 °C, and the normal boiling point is 57.7 °C. What is the enthalpy of vaporization (ΔHvap) for SiCl4 in kJ/mol?

35.7 kJ/mol

45.3 kJ/mol

31.4 kJ/mol

40.1 kJ/mol

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Verified step by step guidance

To find the enthalpy of vaporization (ΔHvap) for SiCl4, we can use the Clausius-Clapeyron equation, which relates the vapor pressure and temperature to the enthalpy of vaporization. The equation is:

\ln_{2} - \ln_{1} = \frac{- {ΔH}_{vap}}{R} (\frac{1}{T_{2}} - \frac{1}{T_{1}})

, where R is the gas constant (8.314 J/mol·K).

First, convert the temperatures from Celsius to Kelvin. The conversion is done by adding 273.15 to the Celsius temperature. So, T1 = 5.4 °C + 273.15 = 278.55 K and T2 = 57.7 °C + 273.15 = 330.85 K.

Next, identify the vapor pressures at these temperatures. At T1 = 278.55 K, the vapor pressure P1 is given as 100 mmHg. At T2 = 330.85 K, the vapor pressure P2 is the normal boiling point pressure, which is 760 mmHg (since it's the atmospheric pressure at boiling point).

Now, substitute the values into the Clausius-Clapeyron equation:

\ln_{(760 / 100)} = \frac{- {ΔH}_{vap}}{R} (\frac{1}{330.85} - \frac{1}{278.55})

Finally, solve for ΔHvap. Rearrange the equation to isolate ΔHvap and calculate its value in J/mol, then convert it to kJ/mol by dividing by 1000. This will give you the enthalpy of vaporization for SiCl4.