activation energy, in chemistry, the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo chemical transformation or physical transport.
Activation energy is the energy required for a reaction to occur, and determines its rate.
Activation energy is the amount of energy that needs to be supplied in order for a chemical reaction to proceed.
They require a certain amount of energy just to get started. This energy is called activation energy. For example, activation energy is needed to start a car engine. Turning the key causes a spark that activates the burning of gasoline in the engine.
Activation energy = Threshold energy - Average energy of the reactants.
Activation energy is the minimum energy required to cause a reaction to occur. To understand activation energy, we must first think about how a chemical reaction occurs. Anyone who has ever lit a fire will have an intuitive understanding of the process, even if they have not connected it to chemistry.
Activation Energy is the energy which must be provided to potential reactants. Moreover, in a chemical or a nuclear system so that a spark can be given to a chemical reaction or a nuclear reaction.
The minimum quantitiy of external energy required for the conversion of reactant into product or to produce an unstable intermediate is called activation energy. It is E. Rate of reaction is inversely proportional to the activation energy.
In relation to biology (such as biochemistry), the activation energy (or energy of activation) pertains to the energy needed to initiate a reaction. For instance, the activation energy required to breakdown glucose into pyruvic acid in respiration is two ATP.
Activation energy can be thought of as the magnitude of the potential barrier (sometimes called the energy barrier) separating minima of the potential energy surface pertaining to the initial and final thermodynamic state.
The activation energy is the minimum energy required for a reaction to occur. This means that the reactant molecules have enough kinetic energy to collide successfully and overcome the repulsion caused by outer electrons.
Activation energy is defined as the minimum amount of extra energy required by a reacting molecule to get converted into product. It can also be described as the minimum amount of energy needed to activate or energize molecules or atoms so that they can undergo a chemical reaction or transformation.
activation energy. The amount of energy required to cause a chemical reaction;specifically the energy required to reach the transition state.
When reactant molecules absorb energy, their bonds loosened and new loose bonds are formed between them. The intermediate thus formed is called an activated complex or transition state. It is unstable and immediately dissociates to form the stable products.
Fortunately, it's possible to lower the activation energy of a reaction, and to thereby increase reaction rate. The process of speeding up a reaction by reducing its activation energy is known as catalysis, and the factor that's added to lower the activation energy is called a catalyst.
Activation energy is the minimum energy needed for 'successful collisions' where atoms within the reactants rearrange to form products. It can be represented on an energy level diagram. The diagram shows that when a catalyst is used, the activation energy is reduced.
Determining Activation Energy. Notice that when the Arrhenius equation is rearranged as above it is a linear equation with the form y = mx + b; y is ln(k), x is 1/T, and m is -E/R. The activation energy for the reaction can be determined by finding the slope of the line.
The activation energy is the energy required to start a reaction. Enzymes are proteins that bind to a molecule, or substrate, to modify it and lower the energy required to make it react.
In chemistry an activated complex is defined by the International Union of Pure and Applied Chemistry (IUPAC) as "that assembly of atoms which corresponds to an arbitrary infinitesimally small region at or near the col (saddle point) of a potential energy surface".
Threshold Energy: It is the minimum amount of energy which the reactant molecules must possess for the effective collision in forming the products. Activation Energy: It is the excess energy required by the reactants to undergo chemical reaction.
This means that the activation energy is almost always positive; there is a class of reactions called barrierless reactions, but those are discussed elsewhere. For similar reactions under comparable conditions, the one with the smallest E will occur most rapidly.