Melting point of ice decreases with increase in pressure

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SUMMARY

The melting point of ice decreases with an increase in pressure due to the unique properties of water. Unlike most solids, ice expands when it freezes, resulting in a lower density compared to liquid water. This expansion means that under increased pressure, it is energetically more favorable for ice to melt rather than freeze. Consequently, to maintain the melting point under higher pressure, the temperature must decrease.

PREREQUISITES
  • Understanding of phase changes in materials
  • Basic knowledge of thermodynamics
  • Familiarity with the properties of water and ice
  • Concept of pressure and its effects on states of matter
NEXT STEPS
  • Research the Clausius-Clapeyron relation and its implications on phase transitions
  • Explore the thermodynamic principles governing the behavior of water under varying pressure
  • Study the effects of pressure on other materials and their melting points
  • Investigate real-world applications of pressure-induced melting, such as in glaciers and ice skating
USEFUL FOR

Students of physics, chemists, environmental scientists, and anyone interested in the thermodynamic properties of water and ice.

Fiona Rozario
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Can someone please explain why the melting point of ice decreases with increase in pressure?
I understand that generally speaking for a solid, greater the pressure applied, greater energy needed to break the bonds to change state and hence greater the temperature (melting point). What is the case with ice?
 
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Ice expands at it freezes and contracts as it melts. So with increased pressure it is energetically more favorable to melt than to freeze. In order to remain at the melting point, temperature must decrease to compensate for increased pressure.
 

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