Collision theory: Difference between revisions
From Glossary of Meteorology
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<div class="definition"><div class="short_definition">Theory of chemical reactivity that states that only colliding molecules can undergo chemical reaction and then only if their combined [[kinetic energy]] exceeds a critical value.</div><br/> <div class="paragraph">The maximum value for the [[rate coefficient]] for a simple, bimolecular, gas-phase reaction, assuming reaction occurs on every collision, is about 2 × 10<sup> | <div class="definition"><div class="short_definition">Theory of chemical reactivity that states that only colliding molecules can undergo chemical reaction and then only if their combined [[kinetic energy]] exceeds a critical value.</div><br/> <div class="paragraph">The maximum value for the [[rate coefficient]] for a simple, bimolecular, gas-phase reaction, assuming reaction occurs on every collision, is about 2 × 10<sup>-10</sup> cm<sup>3</sup> per molecule per second. Actual rate coefficients are lower due to two effects—the need to overcome an [[energy]] barrier during collision in order for reaction to occur, and a "steric factor," which accounts for the fact that reaction can occur only when the collision occurs in a certain geometry.</div><br/> </div> | ||
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Latest revision as of 13:55, 20 February 2012
collision theory
Theory of chemical reactivity that states that only colliding molecules can undergo chemical reaction and then only if their combined kinetic energy exceeds a critical value.
The maximum value for the rate coefficient for a simple, bimolecular, gas-phase reaction, assuming reaction occurs on every collision, is about 2 × 10-10 cm3 per molecule per second. Actual rate coefficients are lower due to two effects—the need to overcome an energy barrier during collision in order for reaction to occur, and a "steric factor," which accounts for the fact that reaction can occur only when the collision occurs in a certain geometry.
