As one might expect, the temperature of a substance typically increases as energy is added to it. This is the case with most substances in all phases. The exception is when a substance crosses to a different phase, which usually involves no temperature change. The energy difference between these phases is called the “energy of formation”.  

 

Leaving the phase change aside, if we focus on the thermodynamics of a substance in the gas phase alone, we find the temperature versus energy curve often looks something like this.

 

Figure of temperature verses vs enthalpy for nitrogen as calculated by NIST Refprop

Figure of Temperature vs. Enthalpy for Nitrogen as Calculated by NIST Refprop

   

In the first section of the plot, we see the temperature of the gas increases fairly linearly as energy is added in. Here the energy level is quantified by the enthalpy, a useful overall measure of energy level. In this initial region, most of the energy is in the form of translational energy (movement of the molecules) and this is realized directly as temperature. Once the temperature increases beyond a certain point, other effects begin to grow. The first is vibration of the molecules. Next is dissociation of the molecules where the chemical bonds are broken and absorb energy. Lastly, comes ionization, which further absorbs energy at the atomic level. We can see the net effect of these is to the depress rate of temperature rise as energy levels increase. 

 

If we invert the curve and plot temperature versus energy, we get something like this:

 

Figure of enthalpy verses temperature vs for nitrogen as calculated by NIST Refprop

Figure of Enthalpy vs. Temperature For Nitrogen as Calculated by NIST Refprop

 

 

Note the slope of the curve is the change in energy level (dH) with respect to temperature (dT). This is referred to as the specific heat (Cp) and it can clearly change over the range of temperature. Some thermodynamic models capture this effect, and some do not. A perfect gas model (blue line) assumes a linear relationship which, by extension, assumes moderate temperatures. A semiperfect gas model uses empirical data for Cp in the model. A common curve for Cp looks something like this for nitrogen:

 

 Figure of specific heat (Cp) verses temperature vs for nitrogen as calculated by NIST Refprop

Figure of Specific Heat (Cp) vs. Temperature for Nitrogen as Calculated by NIST Refprop

 

Note the increasing value of Cp with increasing temperature. I’ll talk more about modeling approaches to capture this effect in another blog.

 

Blogs in this series:

Fluid Phenomena Primer: Energy Versus Temperature, Specific Heat

Phase Change - Make Mine a Double!

When Perfect is Good Enough - Perfect Gas Models

What's Better than Perfect? Semi-Perfect Gas Models

Going Through a Phase – Modeling Phase Change with Cubics

Getting Real – Advanced Real Gas Models

Fluid Modeling: Liquified

The Ultimate Fluid Model: Non-Equilibrium Modeling