SUMMARY
The entropy change of a 33.0 g ice cube melting in water just above freezing can be calculated using the formula ΔS = Q/T, where Q is the heat absorbed and T is the temperature in Kelvin. For the melting process, Q equals the heat of fusion (334 J/g), resulting in an entropy change of approximately 4.0 J/°C. For the 7.3 g of water evaporating on a hot plate slightly above the boiling point, the entropy change can be determined using the heat of vaporization (2260 J/g), yielding an entropy change of about 10.4 J/°C. Both calculations require understanding of thermodynamic principles and the specific heat capacities involved.
PREREQUISITES
- Understanding of thermodynamic principles, specifically entropy.
- Familiarity with the heat of fusion and heat of vaporization concepts.
- Knowledge of temperature conversion to Kelvin.
- Ability to apply the formula ΔS = Q/T for entropy calculations.
NEXT STEPS
- Research the heat of fusion for various substances.
- Study the heat of vaporization and its applications in thermodynamics.
- Learn about temperature conversion methods, particularly to Kelvin.
- Explore advanced entropy calculations in different phases of matter.
USEFUL FOR
Students and professionals in chemistry, physics, and engineering fields who are studying thermodynamics and entropy changes in phase transitions.