Final answer:
The student's question involves using the Clapeyron equation parameters (the change in entropy and volume) to explain how the melting temperature of a substance is affected by an increase in pressure from 1 bar to 150 bar. The calculation would require the densities and the molar mass, which are not provided numerically, to find changes in volume and enthalpy for the phase change at the melting point.
Step-by-step explanation:
The question refers to the change in melting temperature of a substance as the external pressure is increased from 1 bar to 150 bar, and the need to calculate the clapeyron equation parameters associated with this change.
Since the initial density of the solid and liquid states at the substance's normal melting temperature are not provided numerically in the question, we can't calculate the values explicitly but can discuss the process.
The Clapeyron equation can be used to relate the change in pressure to changes in melting temperature.
It states that the change in pressure with respect to the change in temperature (dP/dT) for a phase change is equal to the change in entropy (ΔS) divided by the change in volume (ΔV), which can also be derived from the enthalpy (ΔH).
To calculate ΔS and ΔV, you would typically need the specific values for densities and molar mass to find the changes in volume and enthalpy associated with the phase change at the melting point.
The densities of liquid and solid phases at a given temperature, combined with the molar mass, can give ΔV, whereas ΔH can commonly be found through calorimetry or derived from known thermodynamic tables.
These values would then be used in the Clapeyron equation to find the slope of the melting curve on a phase diagram, which corresponds to the change in melting temperature as pressure increases.