Abstract: A method for manufacturing a microcrystalline glass, the microcrystalline glass manufactured according to the method, and a use thereof are provided. The method includes: (1) nucleation of a raw glass sheet, followed by primary crystallization, where: the primary crystallization temperature is x1, the primary crystallization time is t, and the primary crystallization temperature x1 and the primary crystallization time t satisfy the following conditions: first, ?a×t+652?x1??a×t+667, where a is a constant, 0.1?a?0.25, and tis 10 to 300 min; and second, y1=0.0029x1+b, where y1 is the glass density after primary crystallization, and 2.440 g/cm3?y1?2.490 g/cm3, b is a constant, and 0.55?b?0.60; and (2) secondary crystallization of the glass sheet which has been subject to primary crystallization.

Abstract: The present disclosure provides methods for producing cathode materials for lithium ion batteries. Cathode materials that contain manganese are emphasized. Representative materials include LixNi1-y-zMnyCozO2 (NMC) (where x is in the range from 0.80 to 1.3, y is in the range from 0.01 to 0.5, and z is in the range from 0.01 to 0.5), LixMn2O4(LM), and LixNi1-yMnyO2 (LMN) (where x is in the range from 0.8 to 1.3 and y is in the range from 0.0 to 0.8). The process includes reactions of carboxylate precursors of nickel, manganese, and/or cobalt and lithiation with a lithium precursor. The carboxylate precursors are made from reactions of pure metals or metal compounds with carboxylic acids. The manganese precursor contains bivalent manganese and the process controls the oxidation state of manganese to avoid formation of higher oxidation states of manganese.

Abstract: The present disclosure provides methods for producing cathode materials for lithium ion batteries. Cathode materials that contain manganese are emphasized. Representative materials include LixNi1?y?zMnyCozO2 (NMC) (where x is in the range from 0.80 to 1.3, y is in the range from 0.01 to 0.5, and z is in the range from 0.01 to 0.5), LixMn2O4 (LM), and LixNi1?yMnyO2 (LMN) (where x is in the range from 0.8 to 1.3 and y is in the range from 0.0 to 0.8). The process includes reactions of carboxylate precursors of nickel, manganese, and/or cobalt and lithiation with a lithium precursor. The carboxylate precursors are made from reactions of pure metals or metal compounds with carboxylic acids. The manganese precursor contains bivalent manganese and the process controls the oxidation state of manganese to avoid formation of higher oxidation states of manganese.

Abstract: A non-pyrophoric AB2-type Laves phase hydrogen storage alloy and hydrogen storage systems using the alloy. The alloy has an A-site to B-site elemental ratio of no more than about 0.5. The alloy has an alloy composition including about (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0. The hydrogen storage system has one or more hydrogen storage alloy containment vessels with the alloy disposed therein.

Abstract: A hydrogen storage system includes a hydrogen storage alloy containment vessel comprising an external pressure containment vessel and a thermally conductive compartmentalization network disposed within the pressure containment vessel. The compartmentalization network creates compartments within the pressure vessel within which a hydrogen storage alloy is disposed. The compartmentalization network includes a plurality of thermally conductive elongate tubes positioned within the pressure vessel forming a coherent, tightly packed tube bundle providing a thermally conductive network between the hydrogen storage alloy and the pressure vessel. The hydrogen storage alloy is a non-pyrophoric AB2-type Laves phase hydrogen storage alloy having: an A-site to B-site elemental ratio of not more than 0.5; and an alloy composition including (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0.

Abstract: A non-pyrophoric AB2-type Laves phase hydrogen storage alloy and hydrogen storage systems using the alloy. The alloy has an A-site to B-site elemental ratio of no more than about 0.5. The alloy has an alloy composition including about (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0. The hydrogen storage system has one or more hydrogen storage alloy containment vessels with the alloy disposed therein.

Abstract: A hydrogen storage system includes a hydrogen storage alloy containment vessel comprising an external pressure containment vessel and a thermally conductive compartmentalization network disposed within the pressure containment vessel. The compartmentalization network creates compartments within the pressure vessel within which a hydrogen storage alloy is disposed. The compartmentalization network includes a plurality of thermally conductive elongate tubes positioned within the pressure vessel forming a coherent, tightly packed tube bundle providing a thermally conductive network between the hydrogen storage alloy and the pressure vessel. The hydrogen storage alloy is a non-pyrophoric AB2-type Laves phase hydrogen storage alloy having: an A-site to B-site elemental ratio of not more than 0.5; and an alloy composition including (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0.

Abstract: A hydrogen storage system includes a hydrogen storage alloy containment vessel comprising an external pressure containment vessel and a thermally conductive compartmentalization network disposed within the pressure containment vessel. The compartmentalization network creates compartments within the pressure vessel within which a hydrogen storage alloy is disposed. One or both of the compartmentalization network and the pressure vessel may be formed by s 3D printing process, such as by Selective Laser Melting (SLM) and/or Direct Metal Laser Sintering (DMLS). The hydrogen storage alloy is a non-pyrophoric AB2— type Laves phase hydrogen storage alloy having: an A-site to B-site elemental ratio of not more than 0.5; and an alloy composition including (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0.

Abstract: A hydrogen storage system includes a hydrogen storage alloy containment vessel comprising an external pressure containment vessel and a thermally conductive compartmentalization network disposed within the pressure containment vessel. The compartmentalization network creates compartments within the pressure vessel within which a hydrogen storage alloy is disposed. The compartmentalization network includes a plurality of thermally conductive elongate tubes positioned within the pressure vessel forming a coherent, tightly packed tube bundle providing a thermally conductive network between the hydrogen storage alloy and the pressure vessel. The hydrogen storage alloy is a non-pyrophoric AB2-type Laves phase hydrogen storage alloy having: an A-site to B-site elemental ratio of not more than 0.5; and an alloy composition including (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0.

Abstract: A non-pyrophoric AB2-type Laves phase hydrogen storage alloy and hydrogen storage systems using the alloy. The alloy has an A-site to B-site elemental ratio of no more than about 0.5. The alloy has an alloy composition including about (in at %): Zr: 2.0-5.5, Ti: 27-31.3, V: 8.3-9.9, Cr: 20.6-30.5, Mn: 25.4-33.0, Fe: 1.0-5.9, Al: 0.1-0.4, and/or Ni: 0.0-4.0. The hydrogen storage system has one or more hydrogen storage alloy containment vessels with the alloy disposed therein.

Abstract: A method for storing and delivering hydrogen gas is described. The method includes reacting a chemical hydride with water in the presence of a synergist. The synergist advances the extent of reaction of the chemical hydride with water to increase the yield of hydrogen production. The synergist reacts with byproducts formed in the reaction of the chemical hydride with water that would otherwise inhibit progress of the reaction. As a result, a greater fraction of hydrogen available from a chemical hydride is released as hydrogen gas.

Abstract: The present disclosure provides methods for producing cathode materials for lithium ion batteries. Cathode materials that contain manganese are emphasized. Representative materials include LixNi1?y?zMnyCozO2 (NMC) (where x is in the range from 0.80 to 1.3, y is in the range from 0.01 to 0.5, and z is in the range from 0.01 to 0.5), LixMn2O4(LM), and LixNi1?yMnyO2 (LMN) (where x is in the range from 0.8 to 1.3 and y is in the range from 0.0 to 0.8). The process includes reactions of carboxylate precursors of nickel, manganese, and/or cobalt and lithiation with a lithium precursor. The carboxylate precursors are made from reactions of pure metals or metal compounds with carboxylic acids. The manganese precursor contains bivalent manganese and the process controls the oxidation state of manganese to avoid formation of higher oxidation states of manganese.

Abstract: High-yield synthesis of higher germanes and higher silanes includes the hydrolysis of a germanium- or silicon-containing alloy with chemical formula AxByGe(Si), wherein A=Mg, Ca, Sr, Ba, Li, Na, K, Rb, Cs, and rare earth metals; B=Al, Si, Sn, Ga, Zn, Fe, Co, Ni, Cu, Ag; x=0-10, y=0-10. The hydrolysis reaction is promoted by an acidic substance such as boron oxide (B2O3), citric acid, hydrochloric acid (HCl), or sulfuric acid (H2SO4). The present invention provides an efficient method of drying higher germanes and higher silanes to prevent their further hydrolysis. Another synthetic process involves the reaction of germanium oxide, borohydride and boron oxide with water. Still another process comprises hydrolyzing the Si1-xGex alloy with a very dilute base solution.

Abstract: The present disclosure provides methods for producing cathode materials for lithium ion batteries. Cathode materials that contain manganese are emphasized. Representative materials include LixNi1-y-zMnyCozO2 (NMC) (where x is in the range from 0.80 to 1.3, y is in the range from 0.01 to 0.5, and z is in the range from 0.01 to 0.5), LixMn2O4(LM), and LixNi1-yMnyO2 (LMN) (where x is in the range from 0.8 to 1.3 and y is in the range from 0.0 to 0.8). The process includes reactions of carboxylate precursors of nickel, manganese, and/or cobalt and lithiation with a lithium precursor. The carboxylate precursors are made from reactions of pure metals or metal compounds with carboxylic acids. The manganese precursor contains bivalent manganese and the process controls the oxidation state of manganese to avoid formation of higher oxidation states of manganese.

Abstract: A method for the production of germane includes reacting an oxide of germanium and/or a non-oxide of germanium compound with a borohydride in a base solution. The method permits production of germane from impure germanium-containing starting materials. Catalysts for the reaction include transition metal elements, as well as oxides, hydroxides, halides, and other complexes or compounds of transition metals. Application of heat increases the efficiency of the catalyst. The methods also include production of germane through oxidation of a pure or impure oxide or non-oxide of germanium. The oxidation is effected by contacting the germanium-containing solid phase starting material with an oxidizing solution. The oxidizing solution may be a basic solution comprising a hydroxide or an acidic solution. The oxidation product of the germanium-containing solid phase starting material is converted to germane through an electrochemical or chemical reduction process.

Abstract: A method for storing and delivering hydrogen gas is described. The method includes reacting a chemical hydride with water in the presence of a synergist. The synergist advances the extent of reaction of the chemical hydride with water to increase the yield of hydrogen production. The synergist reacts with byproducts formed in the reaction of the chemical hydride with water that would otherwise inhibit progress of the reaction. As a result, a greater fraction of hydrogen available from a chemical hydride is released as hydrogen gas.

Abstract: Laves phase-related BCC metal hydride alloys historically have limited electrochemical capabilities. Laves phase-related BCC metal hydride alloys are provided herein with greater than 200 mAh/g capacities and commonly at or greater than 400 mAh/g capacities. By decreasing the temperature or increasing the hydrogen pressure the phase structure of the material a synergistic effect between multiple phases in the resulting alloy is achieved thereby greatly improving the electrochemical capacities.

Abstract: Laves phase-related BCC metal hydride alloys historically have limited electrochemical capabilities. Provided are processes of activating these alloys to produce hydrogen storage materials with greater than 200 mAh/g capacities and commonly much greater than 300 mAh/g capacities. The processes include cooling the alloy during hydrogenation to reduced temperatures or by subjecting the materials to significantly increased hydrogen pressures. Temperatures in many embodiments do not exceed 300° C. By decreasing the temperature or increasing the hydrogen pressure the phase structure of the material is optimized to increase a synergistic effect between multiple phases in the resulting alloy thereby greatly improving the electrochemical capacities.

Abstract: BCC metal hydride alloys historically have limited electrochemical capabilities. Provided are a new examples of these alloys useful as electrode active materials. BCC metal hydride alloys provided include a disordered structure that is formed of a BCC primary phase and three or more electrochemically active secondary phases that are induced to create structural disorder in the system. The structurally disordered hydrogen storage alloys possess unexpectedly superior electrochemical characteristics relative to compositionally similar materials.

Abstract: BCC metal hydride alloys historically have limited electrochemical capabilities. Provided are a new examples of these alloys useful as electrode active materials. BCC metal hydride alloys provided include a pressure plateau in the desorption PCT isotherm measured at 30° C. with center between 0.1 MPa and 1.0 MPa, and/or a plateau region between 0.05 weight percent to 0.5 weight percent of H2. This pressure plateau represents a new catalytic phase capable of producing increased capacity in the absence of additional catalytic phases.