Activation energy: Difference between revisions
Jump to navigation
Jump to search
No edit summary |
No edit summary |
||
| Line 1: | Line 1: | ||
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 | 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 [[Catalysts|catalyst]] or an [http://bms.ncl.ac.uk/wiki/index.php/Enzyme enzyme]. This means that a [[Catalysts|catalyst]] can make a reaction appear to occur faster, as more [[Molecule|molecules]] will have energy greater than activation energy, therefore there are more successful collisions per second. | ||
Revision as of 16:52, 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 molecules will have energy greater than activation energy, therefore there are more successful collisions per second.