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THRESHOLD ENERGY(T.E)
You consider any particular reaction. the molecules of the reactants must necessarily possess certain minimum value of kinetic energy for the collision with other reactant and to from product . this minimum energy that the reactant molecules should possess is known as threshold energy (T.E)
ACTIVATION ENERGY (A.E)
Do you think all the molecules will possess this particular minimum kinetic energy required to form products? obviously not. if you take the graph of no of molecules vs their kinetic energy graph, you will see that only few molecules possess this minimum kinetic energy. so for other molecules also to participate in the reaction you need to provide certain extra energy to them by some means which is known as the activation energy. (A.E)
Now the question arises ,how to calculate the activation energy. suppose in a reaction the average kinetic energy of the molecules of reactant be 10Joules , threshold energy is 50Joules. so what energy should be supplied for all the molecules to react. this is nothing but T.E - Average kinetic energy i.e.,50-10=40Joules. this is what is known as activation energy
so ACTIVATION ENERGY (A.E) THRESHOLD ENERGY (T.E) AND AVERAGE KINETIC ENERGY (K.E) ARE RELATED AS
A.E=T.E - K.E
What else can I help you with?
What term refers to the difference between the energy of the transition state and the energy of the reactants?
The term that refers to the difference between the energy of the transition state and the energy of the reactants is activation energy. It represents the energy threshold that must be overcome for a chemical reaction to occur.
Whats the difference between activation energy and the change of energy in a PE diagram?
Activation energy is the minimum energy required for a reaction to occur, while the change in energy in a potential energy diagram represents the difference in energy between the reactants and the products of a reaction. Activation energy is specific to the transition state of a reaction, whereas the change in energy is a measure of the overall energy difference between reactants and products.
What most likely accounts for the difference between curved a and curve b on the energy diagram?
The reaction described by curve B is occurring with a catalyst.
The difference between catalyst and inhibitor?
A catalyst lower the activation energy (speeds up the reaction) while an inhibitor increases the activation energy (slows it down).
What is another name for the activation energy barrier in a reaction?
The activation energy barrier in a reaction is also known as the energy barrier or energy threshold. This term refers to the minimum amount of energy required for a chemical reaction to occur.
How is activatiokn energy represented on an energy diagram?
Activation energy is represented as the energy difference between the reactants and the transition state on an energy diagram. It is the energy barrier that must be overcome for a chemical reaction to occur. The activation energy is depicted as the peak of the curve on the reaction pathway.
What most likely accounts for the difference between curve A and curve B on the energy diagram?
The difference between curve A and curve B on an energy diagram is most likely due to the activation energy required for the reaction. Curve A likely represents a reaction with a higher activation energy, resulting in a slower reaction rate compared to curve B, which represents a reaction with a lower activation energy and a faster reaction rate.
How does a catalyst increase the rate of a chemical reation?
A catalyst increases the rate of a chemical reaction by providing an alternative pathway with lower activation energy for the reaction to occur. This allows more reactant molecules to reach the activation energy threshold, making the reaction proceed faster. The catalyst itself is not consumed in the reaction and can be reused.
Why is the activation energy pictured as a hill in two diagrams?
The activation energy is represented as a hill in reaction energy diagrams to illustrate the energy barrier that must be overcome for a chemical reaction to occur. The reactants must acquire enough energy to surpass this barrier before they can form products. The height of the hill represents the activation energy required for the reaction to take place.
What role does activation energy play in a chemical reaction, and how can it be represented on a diagram?
Activation energy is the minimum amount of energy required for a chemical reaction to occur. It acts as a barrier that must be overcome for the reaction to proceed. In a diagram, activation energy is typically represented as the energy difference between the reactants and the transition state of the reaction. This barrier must be crossed for the reaction to take place.
What energy is required for the reaction to occur?
Activation energy. The kinetic energy from collisions between particles is used to reach the transition state
What term is used to describe the minimum amount of energy required in order for a reaction to proceed?
This energy is called "energy of activation", it is used to overcame the energy barrier between reactants and products.
