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How does activation energy effect the progress of a reaction?
Activation energy is the minimum amount of energy required to initiate a chemical reaction. A lower activation energy means that more molecules have enough energy to react, leading to a faster reaction rate. Conversely, a higher activation energy requires more energy input and can slow down the reaction rate.
What is an energonic reaction?
It is the opposite of an exergonic reaction. An energonic reaction would be one where more energy is put into the reaction than what comes out of it (like endothermic), while exergonic has more output energy than input (like exothermic).
The smallest amount of energy needed to start a chemical reaction is called?
Technically, it isn't "heat" that makes a chemical reaction happen. "Heat" is merely the flow of energy from one place to another. It is the energy itself that causes a reaction to occur. As an increase in temperature occurs, there is an increase in the energy in a group of molecules by making them mover around faster and bum into each other more. This energy is called "Activation energy", and is defined as the amount of energy required to make the reaction start and carry on spontaneously. Higher activation energy implies that the reactants need more energy to start than a reaction with a lower activation energy. With that being said, activation energy is the answer
If one molecule has more energy than another does it have a higher activation energy?
The activation energy refers to a chemical reaction.
How does activation energy affect the progess of a reaction?
Activation energy is the minimum amount of energy required for a reaction to occur. A higher activation energy barrier means fewer molecules have enough energy to react, slowing down the reaction. Conversely, a lower activation energy barrier allows more molecules to react, leading to a faster reaction rate.
How does activation energy effect the progress of a reaction?
Activation energy is the minimum amount of energy required to initiate a chemical reaction. A lower activation energy means that more molecules have enough energy to react, leading to a faster reaction rate. Conversely, a higher activation energy requires more energy input and can slow down the reaction rate.
How is activation energy related to bond energy?
Activation energy is the minimum energy required for a chemical reaction to occur. It is related to bond energy because breaking chemical bonds and forming new bonds requires energy, which contributes to the activation energy of a reaction. Bonds with higher bond energy are more stable and require more energy to break, hence increasing the activation energy of the reaction.
What does an enzyme do to the activation energy needed to start a chemical reaction?
Enzymes are catalysts, they reduce the activation energy.
Which of the following combinations will generally produce the slowest reaction?
The combination of a low temperature and a high activation energy will generally produce the slowest reaction. A low temperature slows down the kinetic energy of the reacting molecules, while a high activation energy requires more energy for the reaction to occur.
What is an energonic reaction?
It is the opposite of an exergonic reaction. An energonic reaction would be one where more energy is put into the reaction than what comes out of it (like endothermic), while exergonic has more output energy than input (like exothermic).
The amount of energy required to start a reaction is called?
Activation energy. Pg 112 of the living world by Johnson and losos
Do Enzymes increase or decrease the Activation Energy of a Chemical Reaction?
Enzymes decrease the activation energy of a chemical reaction. They do this by providing an alternative pathway with a lower activation energy that allows the reaction to proceed more rapidly.
Which has the highest activation energy?
If the activation energy of a reaction is high, then it requires a large amount of energy to initiate the reaction. The situation arising when a spontaneous reaction has a large activation energy is similar to rolling a ball over a hill. At first, energy must be expended to move the ball to the crest of the hill (or, in the case of a reaction, impart enough energy to the molecules so that their bonds can be sufficiently weakened). However, once the ball is at the top of the hill, it rolls down on its own. This is analogous to the reforming of chemical bonds, which releases energy. High activation energies are typical when a reaction involves molecules whose bonds are strong.
The smallest amount of energy needed to start a chemical reaction is called?
Technically, it isn't "heat" that makes a chemical reaction happen. "Heat" is merely the flow of energy from one place to another. It is the energy itself that causes a reaction to occur. As an increase in temperature occurs, there is an increase in the energy in a group of molecules by making them mover around faster and bum into each other more. This energy is called "Activation energy", and is defined as the amount of energy required to make the reaction start and carry on spontaneously. Higher activation energy implies that the reactants need more energy to start than a reaction with a lower activation energy. With that being said, activation energy is the answer
If one molecule has more energy than another does it have a higher activation energy?
The activation energy refers to a chemical reaction.
What does the activation energy graph reveal about the reaction mechanism?
The activation energy graph shows how much energy is needed for a reaction to occur. A higher activation energy indicates a more complex reaction mechanism with multiple steps, while a lower activation energy suggests a simpler mechanism with fewer steps.
How does activation energy affect the progess of a reaction?
Activation energy is the minimum amount of energy required for a reaction to occur. A higher activation energy barrier means fewer molecules have enough energy to react, slowing down the reaction. Conversely, a lower activation energy barrier allows more molecules to react, leading to a faster reaction rate.
