Collision theory and haber's reaction

O,NO2+NO2---> 2NO2,and so on. The details would depend on the specific conditions and catalyst used, but the overall reaction is the combination of these partial reactions.
  • #1
Entanglement
439
13
N2 + 3H2 -----> 2NH3,

For this reaction to occur does one nitrogen have to collide with 3 hydrogen molecules, or should 3 nitrogen molecules collide with 3 hydrogen molecules to break up the bonds? I just brought up this example because of it's stoichiometry not for any other reason. Thanks in advance.
 
Chemistry news on Phys.org
  • #2
This reaction happens at the surface of some catalyst and is only the net result of some complex series of partial reactions, e.g. adsorption of N2 and H2, dissociation of H2 with the formation of some bonds between the catalyst and H, diffusion of H on the surface, formation of compounds like HN2 forming a complex with the catalyst, addition of further hydrogens, breaking of the N-N bond in some stage, and finally desorption.
 
  • #3
DrDu said:
This reaction happens at the surface of some catalyst and is only the net result of some complex series of partial reactions, e.g. adsorption of N2 and H2, dissociation of H2 with the formation of some bonds between the catalyst and H, diffusion of H on the surface, formation of compounds like HN2 forming a complex with the catalyst, addition of further hydrogens, breaking of the N-N bond in some stage, and finally desorption.
What about 2NO + O2 -------> 2NO2
 
  • #4
ElmorshedyDr said:
What about 2NO + O2 -------> 2NO2

It is probably also a multi step reaction, e.g., NO+ O2---> NO2+O,
NO+O---> NO2
 
  • #5


I can explain that collision theory states that for a chemical reaction to occur, the reacting particles must collide with enough energy and in the proper orientation. In the case of Haber's reaction, the reaction between nitrogen and hydrogen to form ammonia, it is not necessary for one nitrogen molecule to collide with three hydrogen molecules. Instead, it is more likely that three nitrogen molecules will collide with three hydrogen molecules, as stated by the balanced equation.

The stoichiometry of a reaction refers to the ratio of reactants and products in a chemical reaction. In this case, the stoichiometry of Haber's reaction is 1:3 for nitrogen to hydrogen. This means that for every one molecule of nitrogen, there must be three molecules of hydrogen present in order for the reaction to occur.

The breaking of bonds is a result of the collision between the reacting particles, and the energy and orientation of the collision determine whether the bonds will break and a new compound will be formed. So, it is not necessary for a specific number of molecules to collide, but rather for the collisions to have enough energy and proper orientation to result in a successful reaction.

I hope this explanation helps clarify the concept of collision theory and its application in Haber's reaction.
 

FAQ: Collision theory and haber's reaction

1. What is the collision theory?

The collision theory is a theory that explains how chemical reactions occur. It states that for a reaction to take place, particles must collide with each other with enough energy and in the correct orientation.

2. How does the collision theory relate to Haber's reaction?

Haber's reaction is a chemical reaction that converts nitrogen and hydrogen into ammonia. The collision theory explains that for this reaction to occur, nitrogen and hydrogen particles must collide with enough energy and in the correct orientation to form ammonia.

3. What factors affect the rate of a chemical reaction according to the collision theory?

The factors that affect the rate of a chemical reaction according to the collision theory are concentration of reactants, temperature, and surface area. Higher concentrations, temperatures, and surface area increase the frequency and effectiveness of collisions between particles, leading to a faster reaction rate.

4. Can the collision theory be applied to all chemical reactions?

No, the collision theory does not apply to all chemical reactions. Some reactions may not require collisions between particles, such as reactions involving light or nuclear reactions.

5. How can the collision theory be used to increase reaction rates?

To increase reaction rates, the collision theory suggests increasing the frequency and effectiveness of collisions between particles. This can be achieved by increasing the concentration of reactants, raising the temperature, and breaking larger particles into smaller ones to increase surface area.

Similar threads

Replies
8
Views
2K
Replies
7
Views
3K
Replies
8
Views
2K
Replies
6
Views
8K
Replies
2
Views
11K
Replies
2
Views
2K
Replies
4
Views
4K
Back
Top