Effective collision
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Last Update: 2020-11-24
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Source: Internet
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Author: User
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between molecules (or ions) that can cause reactions, called effective collisions. The collision theory holds that
reaction
bio-chemicals must have a molecular collision first, but not every collision can cause a reaction. For example, in hydrogen iodide gas with a concentration of 10 -3 mol/L at
500 degrees C and 101kpa, the number of collisions between molecules is as high as 3.5 × 1028times
/l/s, but the number of effective collisions per unit of time is much smaller, so hydrogen iodide molecules to break down into hydrogen molecules and iodine molecules, will not be completed instantaneously. Molecules capable of effective collisions are called active molecules, but collisions of active molecules are not necessarily effective collisions. Effective collision between reactant molecules must meet two conditions at the same time: First, the reactant molecules must have sufficient momentum to achieve the minimum energy of the active molecules, and second, the reactant molecules must collide with each other in a certain direction, that is, "collision method", in order to cause the old bond to break and form a new bond. The former is an energy factor, while the latter is a spatial factor.
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