What is graphite?
Graphite is an allotrope of carbon, a grayish-black, opaque solid with stable chemical properties and corrosion resistance. Reacting with acids, bases, and other agents takes work. Natural graphite comes from graphite deposits and can also be made from petroleum coke, asphalt coke, and other raw materials through a series of processes to produce artificial graphite. Graphite burns in oxygen to generate carbon dioxide, which can be oxidized by strong oxidants such as concentrated nitric acid, potassium permanganate, etc. It can be used as an antiwear agent and lubricant, and high-purity graphite can be used as a neutron retarder in atomic reactors. It can also manufacture crucibles, electrodes, brushes, dry batteries, graphite fibers, heat exchangers, coolers, electric arc furnaces, arc lamps, pencil refills, etc.
Structure of graphite
Graphite consists of triangular flat carbon sheets. Each layer is called graphene. Carbon atoms are arranged in a honeycomb lattice in each layer, with a bond length of 0.142 nm and a surface spacing of 0.335 nm. The bonding between layers is relatively weak van der Waals bonds and is often occupied by gases, which makes it easy for graphene-like layers to separate and slide through each other. The conductivity perpendicular to each layer is therefore reduced by about 1000 times. The two graphite forms are α (Six Party) and β (Diamond shaped). Their properties are very similar. They differ in the stacking of graphene layers: α The stacking in graphite is ABA, while ABC stacking is energetically unstable and less common β In graphite. α Type can be converted to β Type; when heated to above 1300 ° C, β Type is restored to α Type.
Thermodynamics of graphite
The equilibrium pressure and temperature conditions for the transition between graphite and diamond have been well-established theoretically and experimentally. The pressure varies linearly between 1.7 GPa at 0 K and 12 GPa at 5000 K (diamond/graphite/liquid three-phase point). However, these phases have a wide area near this line where they can coexist. The stable carbon phase is graphite at standard temperature and pressure, 20 ° C (293K), and one normal atmospheric pressure (0.10MPa). At the same time, diamond is metastable, and its conversion to graphite can be ignored. However, at temperatures above approximately 4500 K, a diamond can rapidly convert to graphite. The rapid transformation of graphite to diamond requires a pressure well above the equilibrium line: at 2000 K, a force of 35 GPa is needed.
Price of graphite
Graphite particle size and purity will affect the product's Price, and the purchase volume can also affect the cost of graphite particle. A large amount of large amount will be lower. The Price of graphite particle is on our company's official website.
Graphite supplier
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