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- To think about collision theory, let's consider the following reaction. Here we have atom A reacting with a diatomic molecule B C to form a new diatomic molecule A B and C. According to collision theory, molecules must collide to react. So for this example, atom A has to collide with molecule B C, in order for the reaction to occur.
- 9 min
- Jay
- The molecules can be very large and each have a small portion that can interact. The correct orientation would be the 2 reactive sites exposed to e...
- Actually, 'Exergonic' implies that the change in free energy is negative (i.e. energy flows from the system to the surroundings). But here, we can'...
- The progression of the reaction is basically the same as the time, so it is in some units of time, whether it be minutes, seconds, etc. They aren't...
- Well, if the system is closed (no particles can come inside or go out) then this energy would be converted into heat or movement. If we have the in...
- They reach the activation energy by means of collisions. At a given temperature there is always a distribution of speeds. Some particles are moving...
- Transition state theory describes a hypothetical transition state that exists between reactants and products during a chemical reaction. The specie...
- If activation energy were negative, it would completely invalidate the theory of collisions. Let's say that 2 molecules of different elements colli...
- That is because this example is an *exothermic reaction* where the products are *thermodynamically more stable* than the reactants. It could just a...
- I think you're confunding the analogy with the real concept... When you give enough energy to the system, the mollecules will collide enoughly so t...
Jul 14, 2017 · This video explains how particles collide for a reaction to occur and how this process affects the rate of a reaction. For more free educational resources, v...
- 2 min
- 25.8K
- Lincoln Learning Solutions
Dec 12, 2022 · This video introduces the concept of rate of reaction, followed by how it is measured, graphed, and perceived on a molecular level. It then explores what act...
- 6 min
- 2145
- Tiber Tutor
Mar 29, 2019 · This revision summary video looks at all you need to know about rates of reaction:1. The two practicals you need to know inside out2. Collision theory3. Rate...
- 9 min
- 1230
- Mr Barnes
Collision theory says that particles must collide in the proper orientation and with enough kinetic energy to overcome the activation energy barrier. So let's look at the reaction where A reacts with B and C to form AB plus C. On an energy profile, we have the reactants over here in the left.
- 7 min
- Jay
The collision theory helps explain why certain factors, such as temperature, concentration, surface area, and the presence of a catalyst, affect the rate of a reaction. For instance, increasing the temperature increases the kinetic energy of the particles, leading to more frequent and more energetic collisions, thus increasing the rate of reaction.
People also ask
How does collision theory work?
How many collisions produce a reaction?
Do more collisions mean a faster reaction rate?
Why is collision theory important in chemical reactions?
The first step in the gas-phase reaction between carbon monoxide and oxygen is a collision between the two molecules: CO(g)+O2(g) → CO2(g)+O(g) CO ( g) + O 2 ( g) → CO 2 ( g) + O ( g) Although there are many different possible orientations the two molecules can have relative to each other, consider the two presented in Figure 18.5.1.
