Thanks, it seems to have at least one of the answers. It is way out of my comfort zone so I will have to study it for engineering rather than academic truths. Thanks again.mjc123 said:Try http://www.nrcresearchpress.com/doi/pdf/10.1139/v71-038
I suspect it would be rather corrosive though.
The latent heat of crystallisation of sodium chlorate is the amount of heat energy required to convert one unit of liquid sodium chlorate into its solid form at a constant temperature and pressure.
The latent heat of crystallisation of sodium chlorate can be determined through experiments where the heat energy released or absorbed during the phase change from liquid to solid is measured.
The factors that affect the latent heat of crystallisation of sodium chlorate include temperature, pressure, and the purity of the substance. Higher temperatures and pressures typically result in a lower latent heat, while impurities can affect the strength of the bonds between molecules and therefore change the amount of energy needed for the phase change.
The latent heat of crystallisation of sodium chlorate is important in various industrial processes such as freeze drying and refrigeration. It is also a crucial factor in understanding the physical properties of sodium chlorate and its behavior in different environments.
The latent heat of crystallisation of sodium chlorate is relatively low compared to other substances due to its ionic nature. For example, the latent heat of crystallisation of water is much higher because of the strong hydrogen bonds between its molecules.