Phase Change & Temperature: What's the Difference?

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SUMMARY

The discussion clarifies the distinction between temperature change and phase change in substances. It establishes that during a phase change, such as ice melting, the temperature remains constant despite the absorption of heat. This is due to the energy being used to break intermolecular forces rather than increasing kinetic energy. The key takeaway is that temperature changes and phase changes cannot occur simultaneously in a substance.

PREREQUISITES
  • Understanding of thermodynamics principles
  • Knowledge of phase transitions (e.g., melting, boiling)
  • Familiarity with kinetic molecular theory
  • Basic concepts of heat transfer
NEXT STEPS
  • Research the specifics of phase transitions in different substances
  • Explore the role of intermolecular forces in phase changes
  • Learn about the heat of fusion and heat of vaporization
  • Investigate temperature-heat relationships in thermodynamic systems
USEFUL FOR

This discussion is beneficial for students of chemistry, physics enthusiasts, and educators seeking to deepen their understanding of thermodynamic processes and phase changes.

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"When a substance absorbs or releases heat, one of two things can happen: either its temperature changes or it will undergo a phase change but not both at the same time"

Can someone clarify this statement? During a phase change, isn't what's going on really just increasing the kinetic energy of the molecules so intermolecular forces break and thus increasing the temperature of the matter?

Thanks.
 
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No. Phase change occurs in one temperature - like ice melting. As long as there is a mixture of ice and water adding heat will melt the ice, but temperature of the mixture remains constant. It is breaking of the forces that kept molecules in solid (liquid) together that consumes the heat.
 

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