Collision Theory: Definition and Factors that Influence Reaction Rates
Collision Theory: Definition and Factors that Influence Reaction Rates – Have you ever heard of the term Collision Theory? For Physics students, of course this is not a foreign term. But for those of you who don't understand what it means, it's better to read the article below to get to know it better. Let's look at the discussion.
Collision Theory: Definition and Factors that Influence Reaction Rates
Collision theory is a qualitative explanation of how a chemical reaction can take place and why the reaction rate can be different for different reactions. The collision theory was first proposed by Max Trautz in 1916. Max stated that when reactant particles collide with each other, only a few percent of the collisions cause chemical changes known as effective collisions.
In order for effective collisions to occur, the orientation of the molecular collisions must be correct. Orientation is the direction or position of intermolecular collisions. Before a collision occurs, the particles require a minimum energy known as activation energy (Ea). Activation energy is the minimum energy required for a reaction to take place. This energy is used to break bonds as well as form new bonds, resulting in reaction products being formed.
Moving molecules will have kinetic energy. If the movement is faster, the greater the kinetic energy is converted into vibrational energy. If the initial kinetic energy is large, the colliding molecules will vibrate strongly, resulting in the breaking of several chemical bonds in the molecules. The formation of reaction products begins with the breaking of bonds as the first step. However, if the initial kinetic energy is small, the molecules will just bounce around and be intact. For a reaction to occur, a minimum collision energy must be met. Therefore, for a reaction to occur, the colliding molecules must have a total kinetic energy equal to or greater than the activation energy (Ea). If the kinetic energy is less than the activation energy, the molecules will remain intact, resulting in no reaction occurring.
Chemical reactions occur when particles of reacting substances (reagents) collide with each other. However, not all collisions that occur will produce new substances. New substances can be produced from perfect collisions. A perfect collision is called an effective collision. Substance particles that collide with each other sometimes do not immediately turn into a resulting substance. These collisions first form a complex molecule called an activated complex molecule. The formation of activated complex molecules is related to activation energy. Activation energy (EA) is the lowest collision energy required for the formation of activated complex molecules so that the reaction can take place.
Basic Collision Theory
Collisions that produce reactions are collisions between particles that have energy greater than the activation energy. The smaller the activation energy value, the faster the reaction takes place.
The reaction P + Q → R + S can occur if P + Q has minimum activation energy. The existence of a minimum activation energy allows collisions to occur that produce energy, provided that the collision energy of the reactants is > Ea.
The collision theory based on the kinetic theory of gas molecules states the following things.
- Gas consists of gas molecules that are smaller than the intermolecular distance.
- Gas molecules always move straight in all directions.
- Collisions between gas molecules and the walls of the container are perfectly elastic, meaning that the gas molecules will be reflected back without losing energy.
- The speed of movement of gas molecules is influenced by changes in temperature. The higher the temperature, the faster the gas molecules move.
- The average kinetic energy of gas molecules is the same at the same temperature or is not affected by their mass.
- The reaction rate of a chemical reaction is influenced by several factors. We can control the reaction rate by changing the factors that influence the reaction rate. However, keep in mind that for experimental data with variations in several factors, not all factors always have an influence.
Factors Affecting Reaction Rates
Factors Affecting Reaction Rates
Concentration
Concentration is related to the frequency of collisions. The concentration continues to increase, until there are many reacting substance particles. As a result, perhaps the collisions between reactant particles will continue to be large and the efficient collisions between particles will also continue to increase. In this way, the response will continue to be rapid.
Surface area
If the surface area continues to be large, it is possible that the contact between the reactants will also continue to be large. This will increase the frequency of collisions so that more efficient collisions will occur. Increasing the frequency of efficient collisions will increase the response rate.
Temperature
When the temperature is increased, the kinetic energy in the reactant molecules also increases. The presence of large kinetic energy causes intermolecular movements to continue to be lightning and random. As a result, the frequency of collisions that occur continues to become greater, and the efficient collisions will also continue to increase so that the response continues to occur quickly.
Catalyst
A catalyst is a substance that can speed up the rate of response without undergoing permanent chemical changes so that at the end of the response the substance can be recovered. Catalysts are divided into 2, namely homogeneous catalysts and heterogeneous catalysts.
A homogeneous catalyst is a catalyst that has the same phase as the reactant phase. On the other hand, a heterogeneous catalyst is a catalyst that has a different phase from the reactant phase. Usually heterogeneous catalysts are used in solid form. Meanwhile, the reactant is in the form of gas.
The accumulation of catalyst causes bonus response stages that provide other pathways with lower activation energy (Ea). Activation energy (Ea) is the minimum energy that must be possessed or given to particles so that their collisions produce a response. The bonus response stages take the form of a catalyst binding session and a catalyst release session at the end of the response. Catalysts have special characteristics, meaning they can only act as a specific response.
The catalyst's role is to reduce the activation energy. The presence of a catalyst will cause the response to take place over several sessions. The series of response stages in a chemical response is called a response mechanism. The response session is very slow in a response mechanism, namely the response rate determining session.
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