Why is the molar enthalpy the vaporization that a substance larger than that is molar enthalpy of fusion (at constant pressure); because that example, in the case of ice and water.

You are watching: Why is heat of vaporization greater than fusion  Enthalpies the phase alters are fundamentally associated to the electrostatic potential energies between molecules. The first thing you need to recognize is:

There is one attractive force in between all molecules at long(ish) distances, and a repelling pressure at brief distances.

If you make a graph of potential power vs. Distance between two molecules, it will certainly look something prefer this: Here the y-axis to represent electrostatic potential energy, the x-axis is radial separation (distance in between the centers), and the spheres are \"molecules.\"

Since this is a potential energy curve, you have the right to imagine the system as if it to be the surface ar of the earth, and gravity to be the potential. In other words, the white molecule \"wants\" to roll under the valley until it sits alongside the gray molecule. If it were any closer than just touching, it would need to climb increase another very steep hill. If you try to pull them away, again you have to climb a hill (although the isn\"t as tall or steep). The an outcome is that unless there is enough kinetic energy for the molecule to relocate apart, they often tend to pole together.

Now, the potential energy role between any kind of two types of molecules will be different, however it will constantly have the same an easy shape. What will adjust is the \"steepness,\" width, and depth the the valley (or \"potential power well\"), and the slope of the infinitely lengthy \"hill\" come the appropriate of the well.

Since we are talking about relative enthalpies of fusion and vaporization for a given system, we don\"t need to worry around how this changes for various molecules. We just have to think around what it means to vaporize or melt something, in the paper definition of the spatial separation or relativity of molecules, and also how the relates to the form of this surface.

First let\"s think around what happens once you include heat come a device of molecule (positive enthalpy change). Warmth is a deliver of thermal energy in between a warm substance and a cold one. The is identified by a readjust in temperature, which means that as soon as you include heat come something, the temperature rises (this could be common sense, but in thermodynamics it is necessary to be an extremely specific). The key thing we should know around this is:

Temperature is a measure of the median kinetic energy of all molecules in a system

In other words, as the temperature increases, the average kinetic power (the speed) of the molecules increases.

Let\"s go earlier to the potential energy diagram between two molecules. You recognize that power is conserved, and so ignoring losses as result of friction (there won\"t be any for molecules) the potential energy that deserve to be gained by a fragment is equal to the kinetic energy it started with. In various other words, if the fragment is in ~ the bottom the the well and has no kinetic energy, it is not going anywhere: If the literally has no kinetic energy, we space at absolute zero, and also this is an ideal crystal (a solid). Actual substances in the genuine world constantly have some thermal energy, for this reason the molecule are always sort that \"wiggling\" approximately at the bottom of their potential power wells, also in a solid material.

The concern is, just how much kinetic power do you must melt the material?

In a liquid, molecules are complimentary to move yet stay nearby together

This way you need enough energy to permit the molecules climb up the fine at least a small bit, so that they have the right to slide roughly each other.

If we draw a \"liquid\" heat approximating how much energy that would certainly take, it could look something like this: The red line reflects the typical kinetic energy needed for the corpuscle to traction apart simply a tiny - enough that they have the right to \"slide\" around each various other - but not so lot that there is any far-reaching space in between them. The height of this line compared to the bottom that the well (times Avogadro\"s number) is the enthalpy the fusion.

What if we want to vaporize the substance?

In a gas, the molecules are totally free to move and are really far apart

As the kinetic energy increases, ultimately there is enough that the molecules deserve to actually paris apart (their radial separation can approach infinity). The line could look something like this: I have attracted the heat a little bit shy of the \"zero\" point - where the average molecule would acquire to infinite distance - since kinetic energies monitor a statistical distribution, which method that some are greater than average, some are lower, and right about this allude is where enough molecules would have the ability to vaporize that us would contact it a step transition. Depending upon the specific substance, the line might be higher or lower.

In any type of case, the elevation of this line contrasted to the bottom that the fine (times Avogadro\"s number) is the enthalpy that vaporization.

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As you can see, it\"s a lot greater up. The factor is the for melting, the molecules simply need enough power to \"slide\" approximately each other, while for vaporization, they need enough power to totally escape the well. This means that the enthalpy of vaporization is constantly going come be greater than the enthalpy the fusion.