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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.
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.
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.
What does energy hill diagram represents?
An energy hill diagram represents the energy changes that occur during a chemical reaction. It visually shows the difference in energy between reactants and products, with the peak representing the activation energy needed for the 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 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.
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.
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.
What is the relationship between temperature and the activation energy on a graph?
On a graph, the relationship between temperature and activation energy is typically shown as an inverse relationship. As temperature increases, the activation energy required for a reaction decreases. This is because higher temperatures provide more energy to molecules, making it easier for them to overcome the activation energy barrier and react.
Which statement defines activation energy?
Activation energy is defined as the minimum quantity of energy that the reacting species must possess in order to undergo a specified reaction. That means the energy required to activate atoms or molecules.
How is the activation energy related to whether or not collision between molecules is successful?
Generally speaking, the lower the activation energy, the more successful collision between molecules will happen.
