Activation energy
The minimum amount of energy needed for a reaction to take place is called the activation energy.
Exo means 'outside' and thermic means 'heat'. When heat is released in a reaction, its called an Exothermic reaction. Now, answering the question, the energy required for the reaction to occur is less than the total energy released. So, the extra energy gets converted into heat or light. So, yes there is a net release of energy in an exothermic reaction.
The amount of energy a reaction needs to take place is called activation energy. When this much energy is present, a chemical reaction can occur.
When more energy is released than that which is provided, this is referred to as an exothermic reaction.
Standard free energy doesn't change with an enzyme. Rather, the enzyme acts to redirect that reaction in a particular way, lowering the required energy for the reaction to occur but not changing the energy amount involved.
they reduce the activation energy required for the reaction to occur
The chemical term activation energy is the amount of energy required for a chemical reaction to take place. For more information about different chemical contact a scientists or science professor in one's area.
lower activation energy required for chemical reaction to occur
they reduce the activation energy required for the reaction to occur
Activation energy. The kinetic energy from collisions between particles is used to reach the transition state
The minimum amount of energy needed for a reaction to take place is called the activation energy.
Exo means 'outside' and thermic means 'heat'. When heat is released in a reaction, its called an Exothermic reaction. Now, answering the question, the energy required for the reaction to occur is less than the total energy released. So, the extra energy gets converted into heat or light. So, yes there is a net release of energy in an exothermic reaction.
Endothermic
initiates the reaction
The reaction will not occur unless the activation energy is met.
Activation energy is the energy required by a reaction for the reaction to occur. The catalyst lowers the activation energy, making it easier for the reaction to happen.Improvement:A catalyst don't lowers the activation energy. A catalyst creates a alternative route (*) for the same reaction with a lower activation energy.* = as a result of the interaction of the reagents with the catalyst.
by lowering the activation energy of reactions