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recoveries were > 90% in our measurements. Peak power measurements showed high possible power densities of the materials investigated, up to 6 W/g during dehydration and 2 W/g during hydration of Ca(OH)2 and CaO, respectively. CaO as a tendency shows a faster hydration compared to MgCl2*2 H2O. Because of the need to optimize MgCl2 – based materials for applicability and feasibility, whilst being considered of highest relevance for space heating and warm water thermal energy storage [11], we will concentrate on showing and discussing results obtained using this TCM. During dehydration of MgCl2 * 6 H2O, three distinguishable steps are observed, where the material looses two water molecules on each of the first two steps and one water molecules on the third step. Thermal decomposition was not observed below 130°C using TGA/DSC measurements. If heated to temperatures above 130°C, the third step equal to the loss of one more water molecule can be observed, as well as thermal decomposition, starting at around 130°C, when slow heating rates of about 0.1°C / min are used. Unlike the dehydration, the hydration of MgCl2-hydrates shows no distinguishable discrete stages of hydration at 35°C, but a broad peak with slightly decreasing heat flux during the hydration time of approximately 50 minutes, dependent on sample size and water vapour partial pressure. The hydration TGA/DSC graph is shown in figure 2. The graph shows influences of occurring overhydration, as the heat flux does not return to the bottom line and the sample mass keeps increasing as long as the moist gas is flowing into the reaction chamber (in this measurement, 20 min settling time was used until the moist gas was switched on). The water taken up from the moist gas can cause additional steps to occur in dehydration measurements if starting below 30°C. Figure 2: Hydration TGA/DSC plot of MgCl2 * 2 H2O to MgCl2 * 6 H2O (35°C, p(H2O) ~ 2 kPa) We were able to observe a dependency of the peak power on water vapour partial pressure in the reaction chamber, as well as on the thickness of the layer, varied by using different amounts of the samples (figure 3). The highest peak power was observed using an initial amount of 5 mg of MgCl2 * 6 H2O, corresponding to a thickness of the layer of approximately 2 mm. The lower peak power of the 2.5 mg sample is due to a higher influence of heat dissipation which must be regarded as a possible source of errors using this method, the lower peak power of the 7.5 mg and 15 mg samples are due to the higher thickness of the layers. The error bars show variation in resulting water vapour partial pressures using the described setup as well as the variation of several hydration/dehydration cycles using the same sample. As can be seen from the two measurements using 5 mg of MgCl2 * 6 H2O, the repeatability of the hydration experiments may depend on different levels of compression of the samples when introduced into the alumina crucible.PDF Image | THERMOCHEMICAL STORAGE MATERIALS RESEARCH
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