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Start up energy of a chemical reaction?
The activation energy is the minimum amount of energy required to initiate a chemical reaction. It helps to break the existing bonds in reactant molecules and start the formation of new bonds in the product molecules. Lowering the activation energy can increase the reaction rate.
What is the effect of a catalyst on the required energy to achieve effective collisions?
A catalyst lowers the activation energy required for a chemical reaction to occur by providing an alternative reaction pathway with lower energy barriers. This makes it easier for reactant molecules to collide effectively and react to form products.
Which is the best description of activation energy?
Activation energy is the minimum amount of energy required for a chemical reaction to occur. It is needed to initiate the reaction by breaking the bonds of the reactant molecules.
What are the molecules that bump into one another cause energy called what?
The molecules that bump into one another and cause energy are called reactants. When reactant molecules collide with enough energy, they can undergo a chemical reaction and transform into products. This collision energy is known as activation energy.
Why are catalysts spread out in a reaction?
Catalysts are spread out in a reaction to increase the chances of them coming into contact with the reactant molecules. By increasing the surface area of the catalyst, more reactive sites are available for the reactant molecules to bind to, which helps to speed up the reaction.
How do changes in temperature affect the rate of a reaction?
Increasing temperature generally increases the rate of a reaction because it provides more energy for the reactant molecules to overcome activation energy. Lowering the temperature can slow down the reaction as there is less energy available for the reactant molecules to collide effectively and form products. However, extreme temperatures can denature enzymes and disrupt the reaction process.
What must be overcome to get a reaction started?
To get a reaction started, the activation energy must be overcome. This energy barrier is necessary to break the bonds in the reactant molecules and initiate the reaction. Once the activation energy is surpassed, the reaction can proceed on its own.
Start up energy of a chemical reaction?
The activation energy is the minimum amount of energy required to initiate a chemical reaction. It helps to break the existing bonds in reactant molecules and start the formation of new bonds in the product molecules. Lowering the activation energy can increase the reaction rate.
What is the difference between an effective collision and ineffective collision of reactant particles?
An effective collision between reactant particles results in a chemical reaction, while an ineffective collision does not lead to a reaction because the particles do not have enough energy or correct orientation to break and form bonds. In an effective collision, reactant molecules collide with sufficient energy and in the correct orientation to overcome the activation energy barrier and form product molecules.
What is the effect of a catalyst on the required energy to achieve effective collisions?
A catalyst lowers the activation energy required for a chemical reaction to occur by providing an alternative reaction pathway with lower energy barriers. This makes it easier for reactant molecules to collide effectively and react to form products.
Can a reaction have zero activation energy?
No, all reactions require some activation energy to proceed, even if it is very small. Activation energy is the minimum amount of energy required for reactant molecules to transform into product molecules.
Which is the best description of activation energy?
Activation energy is the minimum amount of energy required for a chemical reaction to occur. It is needed to initiate the reaction by breaking the bonds of the reactant molecules.
Why does increasing the temperature speed up the reaction?
It provides energy to overcome the activation energy.
What are the molecules that bump into one another cause energy called what?
The molecules that bump into one another and cause energy are called reactants. When reactant molecules collide with enough energy, they can undergo a chemical reaction and transform into products. This collision energy is known as activation energy.
Why does the temperature in a chemical reaction rise?
The temperature in a chemical reaction rises because energy is released as bonds are broken and formed between reactant molecules. This excess energy causes the surrounding molecules to move faster and increases the overall temperature of the system.
What is the definition of activation energy?
Activation energy is the minimum amount of energy required for a chemical reaction to occur. It represents the energy barrier that must be overcome for reactant molecules to transform into products. Higher activation energy results in slower reaction rates.
How much energy do the reactants have?
The energy of the reactants in a chemical reaction is known as the activation energy. It represents the minimum amount of energy required to initiate a reaction by breaking the chemical bonds in the reactant molecules. The reactants typically have higher energy levels than the products in an exothermic reaction.
