Activation energy

From The School of Biomedical Sciences Wiki
Revision as of 16:08, 2 December 2011 by 109292542 (Talk | contribs)
Jump to: navigation, search

The activation energy of a reaction is the minimum amount of energy required to break chemical bonds.  All chemical reactions have an intermediate transition state that is at a higher energy than the reactants. This transition state must be overcomed before the product can form.  This energy can be lowered by the use of a catalyst known asenzymes in  biochemistry. A catalyst lowers the activation energy. This means that a catalyst can increase the speed of a reaction, as more molecules will have an energy greater than activation energy (second transition state). Therefore, there are more successful collisions per second. In enzyme catalysed reactions, enzymes react with substrate to form an enzyme-substrate complex. This enzyme substrate complex lowers the activation energy of the reaction and thus, leads to the formation of products. 

Personal tools