Paraffins or straight-chain alkanes are characterized by the chemical formula C_nH_2n+2 or CH₃–(CH₂)_n–CH₃ (10, 11).Pure paraffin waxes are very expensive, thus only technical grade paraffins are commonly used as PCMs due to cost considerations (10, 21). They are widely utilized as PCMs because of their favorable properties: moderate thermal storage density (approximately 200 kJ/kg and 150 MJ/m³), congruent melting and solidification with negligible subcooling (good nucleating properties), good chemical stability without phase segregation, little volume change, non-corrosive with metal containers, non-toxic and moderate cost (4, 10, 21, 38, 43, 44). They usually show stable properties and good thermal reliability even after 1000–2000 thermal cycles (21). However, they have low thermal conductivity (≈0.2 W/mK), which reduces their heat exchange rate during the melting and solidification processes (1, 38). In addition, they show moderate flammability and can interact with some plastic containers, particularly with polyolefins, leading to infiltrations and softening (1, 10).

Table 7 shows the straight-chain alkanes tested in literature and their performance according to the results obtained by different authors.

The melting point of paraffins increases with the number of alkane chains within the molecule (10, 38), being n-Tetradecane the shortest n-alkane, which melts above 0 °C. Alkanes of different chain length are also prepared in different mixtures to get PCMs with different melting temperatures (48). Table 8 shows examples of mixtures of some alkanes.

The undesirable low thermal conductivity of paraffins and other organic PCMs has been overcome through different solutions such us improved heat transfer by means of metal matrix structures or metallic fins (28, 58, 59), and the development of composite materials based on metal shavings or metal powder embedded in pure PCMs (37, 60).

Along with parrafins, saturated and unsaturated fatty acids have been widely tested and used as PCMs. Saturated fatty acids are characterized by the general formula CH₃(CH₂)_2nCOOH (48). Fatty acids show reproducible melting and freezing behaviour with little or no subcooling (4) and are stable upon cycling since they consist of only one component without the possibility of phase separation (48). Saturated fatty acids also exhibit low phase transition volume changes (21). On the other hand, they show some drawbacks such as low thermal conductivity, mild corrosiveness, and higher cost than technical grade paraffins (approximately 2-2.5 times greater) (10, 48).

Tables 9 and 10 show the tested properties of saturated and unsaturated fatty acids used as LHSMs.

Their melting temperature generally increases with the length of the molecule (1, 48). Different fatty acids can also be mixed to design PCMs with melting temperatures differing from those of the pure fatty acids (48).

Sari and Kaygusuz (66) studied the thermal reliability under 910 thermal cycles of stearic acid, palmitic acid, myristic acid and lauric acid. The percentage of latent heat losses after cycling was 31.9%, 17.8%, 17.1% and 37.2%, respectively, indicating that palmitic acid and myristic acid are more suitable for latent heat storage.

Fatty acid esters are derived from acids in which one hydroxyl (-OH) group is replaced by one alkyl (-O) group (21). They show a narrow temperature range of phase transition and their mixtures can form eutectics with negligible subcooling (1). They are widely available due to their commercial use in other industries (polymer, cosmetics, clothes, etc.) (21). Table 11 shows the tested properties of fatty acid esters used as LHSMs.

Different sugar alcohols and polyalcohols have been tested as potential PCMs. They are characterized by the general formula HOCH₂(CHOH)_nCH₂OH. Sugar alcohols have much higher latent heat of fusion than other organic materials (approximately 300 kJ/kg and 375 MJ/m³). However, they have a high melting temperature (>90 °C) and may be combustive, which limits their application in buildings.

Table 12 shows the tested properties of sugar alcohols used as LHSMs.

Polyethylene glycols (PEGs) are composed of dimethyl ether chains having the hydroxyl group at the end, being characterized by the chemical formula HO–CH₂–(CH₂–O–CH₂–)_n–CH₂–OH or C_2nH_4n+2O_n+1 (21). They are chemically and thermally stable under cycling, non-flammable, non–toxic, non–corrosive and have moderate cost. However, they present low thermal conductivity as other organic materials. Table 13 shows the tested properties of PEGs used as LHSMs. The melting point and latent heat of fusion of PEGs increase with increasing molecular weight (1).

Other organic compounds tested as PCMs are aromatic hydrocarbons, monohydroxy alcohols, ketones, ethers, halogen derivatives, sulphur compounds, amides, dienes, oleochemical carbonates (Table 14). They show a relatively moderate thermal storage density (approximately 100–200 kJ/kg and 100–200 MJ/m³). Most of them have not been studied in detail regarding their applicability as PCMs but could be a valuable alternative to paraffins and salt hydrates, which currently dominate the PCM market.

Salt hydrates are characterized by the general formula: AB·xH₂O, being inorganic salts containing water of crystallization (21). Salt hydrates have higher LHSC and thermal conductivity than organic materials for low-to-moderate temperature applications, approximately 350MJ/m³ and 0.5 W/m K, respectively (15, 38). Also, they are non-flammable and cheaper than paraffins. However, they often present some disadvantages which limit their applicability, such us low thermal reliability for long-operation periods, phase segregation, subcooling and corrosiveness (2, 10, 38, 44). Table 15 shows the properties of the main salt hydrates tested.

Some of the barriers for using salt hydrates can be eliminated or significantly reduced to obtain a long-term thermal cycling material by different techniques. One of the main methods used for preventing segregation and sedimentation is adding thickening agents. The decomposition along the melting process into water and salt with less content of water is mainly due to density difference between salt and water, which leads the lower hydrate (or anhydrous salt) to settle down at the bottom of the container (10). Thus, by adding polymeric or cellulosic gelling materials, such as wooden fibres or attapulgite clays, the lifetime of salt hydrates can be increased up to 1000 cycles without significantly impairing their properties (21, 74). Other methods are based on the addition of water to a hydrate, in the quantity which slightly exceeds the stoichiometric ratio, and mechanical stirring of the mixture (10, 74). Supercooling, which refers to a liquid existing at a temperature lower the melting temperature, can be reduced or eliminated by using nucleating agents, which accelerate the crystallization of supersaturated solutions, such as borax or carbon (90). However, they often reduce the thermal conductivity (21). A list of nucleating agents used in salt hydrates has been reported by Kenisarin (74).

Regarding the corrosion properties of salt hydrates, according to Kenisarin (74), stainless steel is compatible with all salts and mild steels would react only weakly. However, aluminium, copper and brass are not recommended in applications because of their limited resistance.

Some metal compounds have been tested as PCMs for low-to-moderate temperature applications. Most of fusible alloys are based on the combination of bismuth with other metals, such as lead, tin, indium, and cadmium (38). They have high volumetric fusion heat because of their high density (10) and present high thermal conductivity, good thermal stability and reliability, and a negligible volume change during phase change (1, 22, 38). However, their usage in buildings is constrained by their moderate-high melting temperature, scarce availability and very high cost. Table 16 shows the properties of main metals and metal alloys reported.

Different organic-organic eutectics and compositions are found in literature and listed in Table 17. Main tested organic eutectics are based on fatty acid mixtures, such as capric acid + lauric acid (CA + LA), capric acid + palmitic acid (CA + PA), lauric acid–palmitic acid (LA–PA), lauric acid–myristic acid (LA–MA) or myristic acid–stearic acid (MA–SA) (50, 64, 103, 104). Thermo-physical properties of theses mixtures have been tested at different weight combinations by DSC analysis with the aim of identifying the eutectic mixture concentration. It has been shown that the melting temperature and the latent heat in the mixture of these materials follow a downtrend process through different concentrations until the eutectic proportion is achieved (64, 67, 105–107).

Organic-inorganic eutectics and compositions tested are listed in Table 18. They are mainly based on the mixture of urea and salt.

Different inorganic-inorganic eutectics and compositions are listed in Table 19. Main inorganic eutectics are based on alloys of salt hydrates.

Adsorption is based on the binding of a gas or liquid on the surface of a porous media (39). Adsorbents are highly porous solids. Since different molecules interact differently with the adsorbent, it is eventually possible to separate them (114). During the energy charging step (desorption process), heat added to the system is used to remove the gas or liquid molecules, for instance water, from the solid surface. When energy is needed the reverse reaction (adsorption) is promoted by adding water to the surface and the stored heat is released. An advantage of the sorption materials in comparison with PCMs is that, in the former, the energy release process can be designed to provide a cooling effect from the evaporator in summer or heating from the reactor in winter, whereas in the case of PCMs the fixed discharging temperature imposes a restriction on their application (17).

The desorption-adsorption storage process can be carried out in both open and closed configurations. Closed configurations mainly consist of two vessels, a reactor and a condenser-evaporator where water is stored. Higher temperatures for heating applications as well as lower temperatures for cooling can be reached in closed systems as compared to open systems. On the other hand, the pressure in the adsorption and desorption processes play a critical role. Thus, closed sorption systems present several benefits form a design point of view. Moreover, the energy density is lower compared to open systems since the adsorptive must be also stored. In open configurations, only water can be used as sorbate. Abedin et al. (115) developed a comparison between both types of thermochemical systems and concluded that the overall energy efficiency was 50 and 69% for closed and open systems, respectively.

Since the adsorption equilibrium is given by specific operating conditions (composition, temperature and pressure), by changing one of these parameters it is possible to regenerate the adsorbent. Thus, information about the adsorption equilibrium of the distinct species is vital to design and model adsorption processes (116). Most studied materials for energy storage by means of adsorption are zeolites and silica gel. New materials such as aluminophosphates (AlPOs) or metal-organic frameworks (MOFs) have been proposed (17, 117). Differences between zeolites and silica gel are related to their structure; while zeolites present a narrow pore size distribution determined by their crystalline structure, silica gel (which is composed of 99% of SiO₂) has a larger range of pore sizes (39).

Silica gel is a desiccant widely used which allows working at a changing temperature bellow 100 °C. One of the main drawbacks for silica gel is that water adsorption occurs at high relative pressures, leading to a low water exchange (17). In the case of zeolites, the main commercial types are Zeolite 4A, 5A, 10X and 13X, which present a desorption temperature usually close to 150 °C (112, 118) that limits their application to low temperature solar systems.

Adsorption of water vapour in both silica gel and zeolite compounds has been investigated experimentally in several works (39, 112). Experiments have shown an almost linear relation between air temperature and humidity at system exit when fixed adsorption conditions are considered (39). Thus, by increasing the humidity ratio (kg H₂O/kg material), air temperature is reduced in the energy releasing step. Regarding to the breakthrough curve, zeolite reaches its maximum outlet temperature which is kept almost constant until adsorption is over whereas in the case of silica gel the outlet temperature falls just after reaching its maximum (39).

Silica gel and zeolites have been tested in several research projects such as the HYDES and MODESTORE projects (2003–2012) (112, 119), which aim at the application of seasonal storage of solar thermal energy for space heating. For the material combination of silica gel and water, test results showed that the temperature lift is sufficient up to a water content in silica gel of about 13%. On the other hand, water contents of less than 3% are not realistically achievable given the temperature attainable from flat plate solar collectors and the temperature of an available heat sink. Therefore, the material has to operate between these limits of water content (3-13%). That means that the storage density of the material is significantly lower than initially expected. Lim et al. (120) built a lab scale closed loop system based on silica gel-water, in which the water uptake is approximately 29.8–56.7% the theoretical value. Sapienza et al. (121) studied the equilibrium and dynamics of the silica gel-water system by using Siogel, a commercial adsorbent. A water uptake of 12% was achieved. Deshmukh et al. (122) carried out thermal analysis of a closed silica gel-water system with the aim to develop a 18kWh storage system at an average temperature lift of 25 °C. Results showed that for these conditions 350 kg of adsorbent are necessary, with an energy storage density of 151 MJ/m³. Fernandes et al. (123) carried out simulations to evaluate a silica gel-water adsorption system which serves as TCES for a conventional solar system. Results indicated that annual energy savings up to 16% can be achieved in comparison with a conventional (water) storage system.

Results achieved with zeolites have shown a better performance due to its high water uptake compared to silica gel, which provides a high energy storage density. According to (112), Zeolite 13 X has a higher water vapour uptake rate than Silica gel 490 (up to 32% of its dry weight). Thus, Zeolite 13X, which was identified as one of the best adsorbents, has been also tested within international projects, such as E-Hub project (2010-2014) or COMTES project (2012-2016). Hauer et al. (124) developed and tested an open adsorption system based on zeolite 13X which provides heat to a district heating facility. Reported results showed an energy storage density of 446 MJ/m³. A domestic hot water system with storage based on zeolite 13X-water vapour was developed and tested by Köll et al. (125). Results demonstrated that an energy density of 640 MJ/m³ can be achieved, which allows achieving a solar fraction of 83.5% for both hot water and space heating. Tatsidjodoung et al. (126) also constructed a prototype using Zeolite 13X/H₂O as the reactive pair, which was validated by means of a 1D mathematical model. Results on discharging process showed that, with a 40 kg zeolite system, an average temperature lift of 38 °C at the exit of zoolite vessel was attained during a period of 8 hours. As in similar prototypes, temperatures up to 180 °C were necessary to carry out the charging process. Analysis on the kinetics of the adsorption process for zeolite 13X/H₂O showed that slow reaction rates reduce the efficiency significantly albeit only below a threshold value for the kinetics coefficient, which for the selected conditions was 0.001 [1/s] (127).

Table 20 shows the main solid adsorbents tested as TSMs. As shown, most of them present a discharge temperature below 70 °C and therefore an efficient low-temperature terminal heating system, such as underfloor heating, is fundamental. Regarding the charging step, thermal energy sources at temperatures of up to 180 °C for Zeolite and 95 °C for Silica gel are needed. Energy density of these TSMs varies between 151 and 648 MJ/m³, which is quite high in comparison with water-based sensible heat systems, although an optimized infrastructure must be designed to reduce the volume of external equipment, such as tanks, pumps, blowers or heat exchangers.

The sorption process in absorption materials is based on liquids, which absorb the gas (usually water vapour) releasing the previously stored energy. In general, liquid materials present higher energy density than solid adsorption materials. However, the energy storage of the prototype decreases significantly in absorption systems since the storage in tanks of liquid must be considered. An advantage of liquid absorption materials is that they can be pumped and used directly as heat transfer fluid, which helps reduce the heat losses. The main components of an absorption process for energy storage are: a desorber and an absorber, a condenser and an evaporator, two solution storage tanks (diluted and concentrated solution) and an absorbate storage tank (134). The operating principle of a stored renewable energy based on liquid absorption materials for heating is: when energy is available (solar in most of cases) an aqueous solution is pumped from the tank to the desorber, where energy input is used to increase the vapour pressure to reach equilibrium. After that, if energy input continues, the solution becomes concentrated as water vapour is released, which is condensed and stored in a water tank. When energy is needed, the concentrated solution is sent to the absorber while water is pumped from the storage tank to the evaporator producing water vapour, which is absorbed by the solution, being the released heat used for air-conditioning proposes.

Several materials have been tested in closed absorption cycles for TCES, such as LiCl, NaOH, CaCl₂ and LiBr. Main properties of these liquid absorption materials are shown in Table 21.

Based on LiCl salt absorption process, a thermo-chemical accumulator (TCA) was patented by Olsson et al. (147), which is currently at the commercial level for cooling applications. TCA consists of a three-phase absorption process (solid, solution and vapour). The system works in batch mode. Water is desorbed from the solution in the charging mode and causes the solution saturation followed by the formation of solid crystals that fall under gravity into the vessel. In discharging mode, the saturated solution is pumped to a heat exchanger where it absorbs vapour coming from the evaporator, whose energy input is taken either from the environment (heating application) or from the building (cooling) (148). After that, the unsaturated solution passes though the crystals zone to reach saturation again before being stored. The condensation heat and released binding energy is transferred to the environment (cooling mode) or to the building (heating mode) (148). Laboratory test results showed an energy density for the material, LiCl salt, of 911 MJ/m³, although considering the entire TCES prototype the energy density results around 306 MJ/m³ (112). Hui et al. (149) evaluated seven absorption systems from an energy storage point of view. Results showed that the LiCl/H₂O couple has an excellent storage capacity and efficiency, with the disadvantage of a high cost compared to other liquid absorbents (more than 14 times higher than CaCl₂). Nevertheless, the high energy density of the LiCl-based system makes it an attractive choice from a storage capacity cost perspective resulting in one of the materials with lower cost per kWh stored (~6€/kWh) (150).

In the case of the NaOH system, a prototype for heating has been tested (112). The system works as a heat pump in which the driving force is the difference of the vapour pressures above water and NaOH solution (soda lye). In this system configuration, contrary to the TCA described above, the tanks are separated and works as a continuous process. Test results showed a good kinetics at desorption temperatures of 120 °C. The energy density of the system and prototype are 900 and 18 MJ/m³ respectively, but this prototype can be highly improved with an optimized system design (112). Another test carried out by Weber et al. (135) showed that, including tanks and heat exchangers, the total energy density could be three times higher compared to traditional hot water storage at 70 °C, and about six times higher for a tap temperature of 40 °C for low-temperature space heating. Fumey et al. (140) tested at lab-scale a conventional spiral fined tube heat exchanger where the absorbent (NaOH) flows along the fin from top to bottom. A temperature lift of 35 °C between the maximum absorbent temperature and the absorbate was measured, with a dilution from 50wt% to 27wt%. During desorption a concentration lift from 25wt% to 53wt% is achieved, which translates into a theoretically energy density of 1566 MJ/m³.

CaCl₂-based system behaviour was analysed by Davidson et al. (98) for its use as liquid desiccantin an atmospheric-pressure chiller. Solar energy is stored in a liquid CaCl₂ volume by heating the solution and vaporizing H₂O. Energy is extracted as water is reabsorbed and/or the solution is cooled (142). The energy density of the material, which is dependent on how the tank is discharged, is 106 kWh/m³, similar to that of LiCl for the same operating parameters (98). Computational results showed that buoyancy driven flow induced by the presence of an immersed heat ex-changer is sufficient to heat and thermally stratify the storage fluid (142). Transport of mass across the density gradient between regions is limited by diffusion. Richter et al. (143) developed an experimental analysis on the absorption system based on CaCl₂. In this work, storage is charged at 130 °C while the reverse reaction allows an energy discharge at 165 °C, which means a thermal upgrade of 35 °C and a thermochemical storage density of approximately 777.6 MJ/m³. Esaki et al. (151) assessed experimentally the use of a chemical heat pump for upgrading waste heat during the hydration of CaCl₂, which occurs within a packed bed reactor. A waste heat temperature upgrading from 100 °C up to 155 °C was achieved with a performance coefficient of 0.48.

Liquid absorbent LiBr was also tested by N’Tsoukpoe et al. (134, 144) as a promising candidate for long-term energy storage in buildings. An 8 kWh energy storage prototype was built based on two storage tanks (water and solution: 88.5 kg) and two falling films heat exchangers (desorber/absorber, condenser/evaporator) assembled to the reactor, which produces a heating power of 1 kW. Several tests were carried out, focused in the charging process under practical conditions (25 °C-95 °C in the desorber and 10–30 °C in the condenser). It was demonstrated that a storage of 13 kWh is possible when charging the prototype with a thermal power of 2-5 kW. Discharging tests indicate absorption temperatures of about 30-40 °C, which can be low for space heating. Xu et al. (145) proposed an absorption solar energy storage system which uses a LiBr solution. A stored energy density of 368 MJ/m³ was achieved. Perier-Muzet and Le Pierres (146) assessed the efficiency of a LiBr/H₂O absorption heat storage system integrated with a solar thermal facility for space heating. They analysed the impact of using a solution heat exchanger (SHX), which could improve both the energy efficiency and storage density up to 75% and 331 MJ/m³, respectively.

Another possibility is using liquid absorption materials for TCES in open systems. During absorption (discharging step) the concentrated solution is sent to an exchange surface where it gets in contact with an air stream. Humidity is removed from air and the solution becomes diluted by the absorption of vapour. During regeneration (reverse process) the solution is again concentrated by the mass and heat transfer with a hot air stream. In open absorption cycles the desiccants are regenerated against the ambient water vapour pressure (dew point of the ambient air) whereas the reference temperature is well above the ambient wet bulb temperature, thus open cycle regeneration requires lower regeneration temperatures and therefore higher collector efficiency (39). An open system based on CaCl₂/H₂O was tested by Bouché et al. (152), which, according to test results, could allow a thermal upgrade of approximately 65 K.

Energy storage by means of chemical reaction materials is based on using the heat obtained from an external source (e.g. solar) to drive an endothermic reaction. The products of the reaction are stored and, when energy is needed, brought together to induce the reversible reaction (exothermic). This group of energy storage materials present a higher energy storage density than previous materials. Main disadvantages could be a low chemical stability after cycling (loss on sorbent capacity) (129), slow kinetics associated to insufficient temperature rise in the reactor (153), and poor heat and mass transfer in gas-solid reactions (154). A number of salt hydrates have been analysed as potential candidates for TCES in buildings such as MgSO₄·7H₂O, MgCl₂·6H₂O and CaCl₂·6H₂O. Table 22 shows the properties of main chemical reaction materials.

MgSO₄·7H₂O is a promising energy storage material with a high energy density (155). A characterization of MgSO₄·7H₂O as TSM was carried out by Bales et al. (112). The results obtained from TGA tests showed that the dehydration of MgSO₄·7H2O occurs in three steps, namely, formation of MgSO₄·6H₂O, MgSO₄·0.2H₂O and finally MgSO_4.

By analysing the DSC curve (112), it is seen that the third step of dehydration (production of MgSO₄) is exothermic, which is contrary to expectations in dehydration reactions (first and second step are endothermic). According to Ruiz-Agudo et al. (158), the reason for the endothermicity of the final reaction is the recrystallization of an amorphous precursor. During hydration, MgSO₄ takes up water to form MgSO₄.6H₂O. If the releasing energy system works at atmospheric pressure, the MgSO₄ could provide energy for heating applications at 25 °C while in a closed system at low pressure a small amount of energy could be released at 50 °C (159). At 50 °C the material is unable to take up water and deliver heat (159). These values are a limitation to the system application for heating purposes. Okhrimenko et al. (160) analysed dehydration of magnesium sulphate at low water vapour pressure and the reaction mechanism. Experimental results showed that the water content in the solid phase after dehydration depends on water vapour pressure and temperature. The equilibrium constant K was found to follow Van’tHoff equation with ∆H=54.3 k/mol H₂O (160). According to Ferchaud et al. (161), the reaction kinetics for the dehydration reactions of MgSO₄·7H₂O could reach a maximum for a water pressure of 50m bar.

Zondag et al. (156) carried out several dynamic tests to analyse the dehydration kinetics of MgSO₄·7H₂O, Al₂(SO₄)3·18H₂O, CaCl₂·6H₂O and MgCl₂·6H₂O. To simulate the charging process, the first three materials were heated to 150 °C to provoke their dehydration while the CaCl₂·6H₂O was dried at 130 °C to avoid side reactions. After that, to release the energy stored, the materials were hydrated with vapour. The authors observed that sulphates had a much lower temperature rise in the reactor than CaCl₂·6H₂O and MgCl₂·6H₂O, which reached a temperature of around 50–68 °C depending on the reactor and vapour temperatures. In view of the results, MgCl₂·6H₂O was selected as the most promising material for energy storage due to its relatively low charging temperature (≥130 °C) and a discharging temperature sufficiently high to yield water heating (≤60 °C), as well as its high energy density (~2GJ/m³) and low price (<1€/kg) (129). MgCl₂·6H₂O was tested in a lab-scale prototype generating 150 W of thermal power (17 l of material and a steam volume flow of 510 l/min), with an effective energy density of 0.5GJ/m³ (129, 156). According to Barreneche et al. (157) the energy involved in the CaCl₂ dehydration process is 1470MJ/m³.

Composite materials, also called composite “salt porous matrix” (CSPM), have been proposed to enhance the reaction kinetics and the poor heat and mass transfer in chemical reaction materials for energy storage. Composite materials usually consist of salt hydrates and an additive with a porous structure that works as host matrix with high thermal conductivity to improve the reaction rate and the heat release. Most studied materials to be used as additive are zeolites (98, 153, 162), metal foam (154, 163), expanded graphite (164–166) and activated carbon (167). Table 23 shows the main properties of several composite materials for energy storage.

A composite material consisting of a reactive mixture of sodium sulphide/water and graphite additives was analysed by Lammak et al. (164), which was filled in a tube-in-tube heat exchanger and operated between high temperature source and a sink temperature of 30-40 °C. The average heating and cooling power were about 3.79 kW and 0.23 kW, respectively. They found that the amount of adsorbed water could be increased drastically by using the graphite-based composite materials. In another work, Mauran et al. (166) analysed a system composed by SrBr₂ implemented with an expanded natural graphite as reactant and H₂O as refrigerant fluid. The prototype reactor, with a total volume of 1m³, was able to store 60kWh and 40kWh in heating and cooling modes respectively. Power released was 2.5kW for heating and 4kW for cooling applications, which was limited by a poor heat and mass transfer. Even though composite materials were expected to improve this issue, the transfer of heat at the inter-face between the consolidated composite and the wall of the exchanger posed a very strong limitation.

Mette et al. (153) proposed a new regeneration strategy for a thermochemical system based on a composite material composed by zeolite (matrix) and CaCl₂, with the aim of reducing the regeneration temperature without affecting energy density. Simulation results showed that it is possible to reduce the regeneration temperature from 180 °C to 130 °C and therefore the process can be driven by solar thermal collectors. This implies a fractional energy saving higher than in the basic process without the proposed regeneration strategy. Wu et al. (169, 170) studied a CaCL₂-silica gel composite material for energy storage. The results indicated that a 30wt% CaCl₂ solution was the most stable and had the highest energy storage capacity: 822MJ/m³ at a charging temperature of 90 °C. In another work, Jabbari-Hichri et al. (171) studied by means of TG/DCS analysis three supporting materials, silica-gel, alumina and bentonite, mixed with a 15%wt of CaCl₂. Results showed that the CaCl₂-silica gel composite material had the highest energy storage density, with a value of 746 kJ/kg.