SUMMARY
The entropy of vaporization (∆S) for water at 100 degrees Celsius can be calculated using the formula ∆S = ∆H / T. In this discussion, the enthalpy of vaporization (∆H) was determined to be 46.2 kJ/mol, which converts to 46200 J/mol. By substituting the temperature of 373.15 K into the equation, the resulting entropy of vaporization is calculated to be 123.8 J/(mol*K), indicating that the value of ∆S must be less than this threshold for the process to be spontaneous.
PREREQUISITES
- Understanding of thermodynamic concepts such as enthalpy (∆H) and entropy (∆S).
- Familiarity with the ideal gas law and phase changes in substances.
- Basic knowledge of temperature conversions, particularly from Celsius to Kelvin.
- Proficiency in algebraic manipulation of thermodynamic equations.
NEXT STEPS
- Study the derivation and implications of the Gibbs free energy equation (∆G = ∆H - T∆S).
- Learn about phase transitions and their thermodynamic properties in detail.
- Explore the concept of spontaneity in chemical reactions and its relation to entropy.
- Investigate the effects of temperature on the entropy of various substances.
USEFUL FOR
Students studying chemistry, particularly those focusing on thermodynamics, as well as educators and professionals seeking to deepen their understanding of phase changes and entropy calculations.