Clausius-Clapeyron equation and enthelpy

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The discussion focuses on using the Clausius-Clapeyron equation to analyze the slopes of solid-gas and liquid-gas coexistence curves at the triple point. It emphasizes the relationship between enthalpy changes during phase transitions, specifically that the slope of the solid-gas curve is greater than that of the liquid-gas curve. Participants highlight the importance of understanding the symbols in the equation and the physical significance of the Clausius-Clapeyron equation. Clarifying these concepts is essential for solving the homework problem effectively. Understanding these relationships is crucial for applying thermodynamic principles accurately.
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Homework Statement


Use the Clausius-Clapeyron equation and \DeltaHsub = \DeltaHfus +\DeltaHvap at the triple point to show that the slope of solid-gas P-T coexistence curve is greater than the slope of the liquid-gas coexistence curve.


Homework Equations


Clausius-Clapeyron: 1/P (dP/dT) = \Deltah/RT^2


The Attempt at a Solution


How does this all relate to the question? I don't understand
 
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If you do not understand the relationship to the question, it suggests that you either do not understand the meaning of the symbols in the question or the meaning of the symbols in the C-C Eqn.

A good starting point is writing out what the C-C Eqn is saying, in words.
 
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