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Heterogeneous catalysis begins when one or more reactants are adsorbed onto the catalyst surface. A typical heterogeneous reaction involves a solid catalyst with liquid or gas reactants. Heterogeneous catalysis involves a catalyst in a different phase than the reactants.
#Define initiater free
The catalyst then separates from C if the catalyst is not destroyed through a secondary process the cycle is free to recommence.Ĭatalysts may be broadly classified as either homogeneous or heterogeneous. At this point the reaction occurs, producing XC, with C being the intended product. The catalyst (X) first combines with reactant A, then adds reactant B, producing XAB. The image below illustrates a reaction in which the combination of reactants A and B produces compound C (A+B=C). They are becoming increasingly prominent - due to their ability to reduce chemical waste - with the rise of sustainable ("green") chemistry.Ī catalyst's mechanism is achieved through the catalytic cycle, which is often visually portrayed as a loop due to the regenerative nature of the process. The vast majority of commercial chemical products use catalysts during their production process. The free energy graph below illustrates how catalyzed reactions reach an identical product by using less energy. In addition to the formation of new paths, catalysts may also reduce energy consumption by stabilizing the reaction through the transition state, as well as temporarily destabilizing the reactants themselves. The video below provides an excellent technical introduction to catalysis and the effect of catalysts on activation energy and reaction rate. Catalytic action can also make it possible to perform chemical processes at lower temperature and/or pressure, thereby reducing fuel resources necessary to provide a special reaction environment. (Although they are not consumed by the process itself, catalysts may be inhibited, destroyed, or similarly deactivated through secondary processes such as coking, dissolution, and evaporation.) Catalysts are useful because the alternate pathways typically use less energy than it would take to activate an uncatalyzed reaction.
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Unlike many reagent chemicals, however, catalysts are not consumed when a reaction occurs.
#Define initiater driver
Even when using multipath I/O to achieve fault tolerance, the device driver switches between different targets or initiators statically bound on physical ports, instead of sharing a static address between physical ports.Image credit: Aron Alpha | FuelCellsEtc | Ellsworth AdhesivesĬatalysts and initiators are chemicals used to start, promote, or slow chemical reactions.Ĭatalysts affect chemical reactions by providing alternative pathways for the formation and breaking of bonds for this reason they are considered a type of reagent. Situations where a single physical port hosts multiple addresses, or where a single address is accessible from one device's multiple ports are not very common, as of 2008. In most of these protocols, an address (whether it is initiator or target) is roughly equivalent to physical device's port. Initiator and target terms are applicable not only to traditional parallel SCSI, but also to Fibre Channel Protocol (FCP), iSCSI (see iSCSI target), HyperSCSI, (in some sense) SATA, ATA over Ethernet (AoE), InfiniBand, DSSI and many other storage networking protocols. See the SCSI host adapter article for a more detailed description of initiator's operation. SCSI initiators are sometimes wrongly called controllers. There is nothing in the SCSI protocol that prevents an initiator from acting as a target or vice versa. Each SCSI address (each identifier on a SCSI bus) displays behavior of initiator, target, or (rarely) both at the same time. As in a client–server architecture, an initiator is analogous to the client, and a target is analogous to the server. Typically, a computer is an initiator and a data storage device is a target.