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A catalyst changes the reaction mechanism to one with a lower activation energy; activation energy is lowered when a catalyst is added
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
The presence of a catalyst affects the activation energy of a reaction by lowering the activation energy, helping the reaction go faster and making it so the reaction does not have to use as much energy to fulfill the products.
yes!. the way the reaction gets faster is because the catalyst absorbs the reactant particles on its surface and weakens their bonds. Reactants particles colliding with weaker bonds actually overcomes the activation energy faster as it is now lower. The only thing a catalyst changes in a chemical reaction is the activation energy, keeping in mind that the catalyst increases the rate of reaction in both forward and backward reaction.
it is important that an enzyme is stabilized because... a) the enzyme reduces the energy required to reach the highest energy of the reaction b) therefore the reduction of activation energy increases the number of reactant molecules with enough energy to reach the activation energy and form the product. c) the enzymes can collide faster with the substrate (also known as lock and key)
A catalyst changes the reaction mechanism to one with a lower activation energy; activation energy is lowered when a catalyst is added
as activation energy decreases, reaction will finish faster (length of reaction decreases)
No, the opposite. The lower the activation barrier the faster the reaction goes. That is how a catalyst speeds up the reaction: by lowering the activation energy.See the Web Links for more information.
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
TBB reacts faster - it has a lower activation energy... :)
The presence of a catalyst affects the activation energy of a reaction by lowering the activation energy, helping the reaction go faster and making it so the reaction does not have to use as much energy to fulfill the products.
It lowers it, so the reaction is faster.
It lowers it, so the reaction is faster.
It lowers it, so the reaction is faster.
A chemical catalyst is a substance that lowers the required activation energy of a reaction. The activation energy is the amount of energy required to "activate" or start a process, this can be in the form of many things, such as heat. A chemical catalyst can be seen as a kind of shortcut in a chemical process to speed things up. A catalyst can also be used to increase the activation energy, so that the reaction will slow down. This is useful for slowing down reactions that are normally too fast to witness.
yes!. the way the reaction gets faster is because the catalyst absorbs the reactant particles on its surface and weakens their bonds. Reactants particles colliding with weaker bonds actually overcomes the activation energy faster as it is now lower. The only thing a catalyst changes in a chemical reaction is the activation energy, keeping in mind that the catalyst increases the rate of reaction in both forward and backward reaction.
I dont understand what do you mean by "move", but I know that a chemical reaction can occure easily when energy of products (Ep) is lower than that of reactants (Er). The activation energy is the absolute value of AE=Ep-Er