Collision theory states that when suitable particles of the reactant hit each other, only a certain amount of collisions result in a perceptible or notable change; these successful changes are called successful collisions. The successful collisions must have enough energy, also known as activation energy, at the moment of impact to break the pre-existing bonds and form all new bonds. This results in the products of the reaction. Increasing the concentration of the reactant brings about more collisions and hence more successful collisions. Increasing the temperature increases the average kinetic energy of the molecules in a solution, increasing the amount of collisions that have enough energy. Collision theory was proposed independently by Max Trautz in 1916 and William Lewis in 1918.
Some reactions occur spontaneously under standard conditions. Some require added energy. This is because it has a higher activation energy. By supplying energy to the system the molecules are moving faster. This means they collide with greater energy and will be able to overcome the activation energy.
Activation energy is the minimum energy that reactant particles must possess in order for the chemical reaction to occur.
That is defined as the energy that must be overcome in order for a chemical reaction to occur. Activation energy may also be defined as the minimum energy required to start a chemical reaction.
It is the amount of energy required for a chemical reaction to take place. This is why some chemical reactions require heat (eg. burning) while others can take place at room temperature (eg. decomposition).
collision theory state that for a chemical reaction to occur , the reacting particles must be:
collide with each other
collide with correct orientation
possess enough amount of energy that is equal to or more than activation of energy
Activation energy is the amount of energy needed to start a reaction. A key factor in the energy of the reaction are the reactants. A factor that will lower the activation energy would be a catalyst.
The energy the molecules must have in order to react
the amount of energy to start a chemical reaction
The energy required for a reaction to begin.
An activation energy, in the realms of chemistry and physics, is the energy required to initiate a reaction.
Explain the effect of molecular polarity on behaviour.
explain the effect of shift reagent in uv on the molecular depostion of organic compound?
Explain why a high energy of activation causes a reaction to be slow?
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Activation energy. Intermediary molecules (catalysts) required.
collision resolution methods
Data packets colliding with one another when being sent through repeaters is an easy way to explain a collision domain. This collision only includes a section of a network.
Explain the effect of molecular polarity on behaviour.
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Explain OSI reference model with revant diag
explain the effect of shift reagent in uv on the molecular depostion of organic compound?
A reference point helps to explain why we are, where we are.
On a switch each port is its own collision domain, therefore collisions do not happen.
Explain why a high energy of activation causes a reaction to be slow?
go on google
yes i can answer it