Activation energy: Difference between revisions
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The activation energy of a reaction is the minimum energy requirement for a successful collision to occur. This energy can be lowered through the use of a catalyst or an enzyme. This means that a catalyst can make a reaction appear to occur faster, as more moleucles will have energy greater than activation energy, therefore there are more successful collisions per second. | The activation energy of a reaction is the minimum energy requirement for a successful collision to occur. This energy can be lowered through the use of a catalyst or an [http://bms.ncl.ac.uk/wiki/index.php/Enzyme enzyme]. This means that a catalyst can make a reaction appear to occur faster, as more moleucles will have energy greater than activation energy, therefore there are more successful collisions per second. | ||
Revision as of 16:04, 11 November 2010
The activation energy of a reaction is the minimum energy requirement for a successful collision to occur. This energy can be lowered through the use of a catalyst or an enzyme. This means that a catalyst can make a reaction appear to occur faster, as more moleucles will have energy greater than activation energy, therefore there are more successful collisions per second.