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Rate of Reaction and Rate Constant
| Content Provider | AK Lectures |
|---|---|
| Description | Let us quickly discuss the collision theory of reactions. In other words, what has to occur for a reaction to actually take place? For the time being, let us suppose that our reaction is exothermic. This basically means that the bonds of the product are more stable and lower in energy than the bonds of the reactants. In order for the starting materials to actually react, they must not only collide with the proper orientation but they must also carry a certain amount of kinetic energy, either at or above the threshold (commonly known as the activation or transition energy). If these starting materials collide with less energy than the energy required to climb the transition state, no reaction takes place. So what exactly is the rate constant of our reaction and how is it related to the actual reaction rate. The rate constant depends on the energy of the transition state (activation energy) and the temperature as shown by the equation in the lecture. If we increase the temperature of the reaction, what we are actually doing is increasing the kinetic energy (the velocity) of the molecules. The reaction rate, also known as rate law, is directly related to the reaction constant. But unlike the rate constant, reaction rate also depends on the concentration of the reactants. In others, we can increase the rate of reaction by increasing the concentration of the reactants. At the same time, we can also increase the rate of reaction by increase temperature and thereby increasing the rate constant. |
| Language | English |
| Access Restriction | Open |
| Subject Keyword | Organic Chemistry orientation product reaction equation collide threshold reactions |
| Content Type | Video |
| Educational Role | Teacher Student |
| Educational Use | Self Learning Lecture Reading |
| Resource Type | Video Lecture |
| Education Level | Under Graduate |
| Subject | Organic chemistry |
