These are all pictured here, it is describing the energy state for a reaction.
http://images.absoluteastronomy.com/images/encyclopediaimages/a/acactivation_energy.svg.png
Free energy refers to the Gibbs energy for a reaction, this is what tells us if the reaction will take place. It is defined as the difference of energy (y-axis) between the initial and final. In order for the reaction to be spontaneous, the final energy state must be lower than the initial.
Activation energy is the amount of energy that must be introduced into the system in order to begin the activation. On the graph, it is the peak. The graph does not have any transition species, but if did they would be denoted by other "hills" in the curve, between the activation and final states.
Catalyst ensures that the activation energy of the molecules is lowered so there is effective collisions,and it does this in two ways;the transition and absorbtion states but inibitors even raises the activation energy and causes in effective collisions.
A catalyst changes the reaction mechanism to one with a lower activation energy; activation energy is lowered when a catalyst is added
Adding a catalyst a chemical reaction can occur with a lower activation energy.
Energy that starts a chemical reaction is called activation energy
initiates the reaction
The energy needed to statr a chemical reaction is the 'Activation Energy' , which is given the symbol (Ea).
An exergonic reaction is activation energy (or energy of activation). An endergonic reaction is essentially the opposite of an exergonic reaction.
Activation energy is the amount of energy needed to start a reaction.
Catalyst ensures that the activation energy of the molecules is lowered so there is effective collisions,and it does this in two ways;the transition and absorbtion states but inibitors even raises the activation energy and causes in effective collisions.
Catalysts are said to reduce the energy of activation during the transition phase of a reaction.
Enzymes lower the activation energy of a chemical reaction.
A catalyst changes the reaction mechanism to one with a lower activation energy; activation energy is lowered when a catalyst is added
The activation energy is decreased by a catalyst.
Activation energy is the amount of energy that a chemical reaction requires to occur.
The Activation Energy.
Activation energy is lowered to speed up a chemical reaction.
A chemical reaction need an activation energy to start.