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The rate of reaction refers to the speed at which the reactants are actually converted to products. While talking about the chemical reactions, some reactions are instant and immediately produce the products, whereas others take time to reach the final equilibrium.
Pressure increases the gases concentration resulting in the increase of the rate of reaction. The reaction rate decreases in the reverse direction and increases in less gaseous molecules direction. Therefore it is clearly understood that Concentration and Pressure are interlinked, and both of them affect the rate of reaction.
The increase in the pressure on a reaction involves the reacting gases increasing the rate of reaction. And modifying the pressure on a reaction involving solids or liquids only has no effect on the reaction rate.
In the case of manufacturing ammonia using the Haber Process, the reaction rate between nitrogen and hydrogen is increased using very high pressures.
H2 (g) + 3H2 (g) ⇌ 2NH3 (g)
And the primary reason to use the high pressures is to enhance the ammonia percentage in the equilibrium mixture, but with this, there is a useful impact on the reaction rate also.
And here comes the explanation for the same
Increasing a gas’s pressure is similar to increasing its Concentration. If you are given a mass of gas, the way to increase the pressure is by squeezing it into a smaller volume. And in the case of the same mass in a smaller volume, then the Concentration is higher.
While mathematically showing the equation, the ideal gas equation becomes,
pV = nRT
Now, rearranging the equation
P = n/V X RT
As RT is constant, as long as the temperature remains constant, the pressure is directly proportional to Concentration. And if you double one, the other will also get doubled.
Talking the two particles, where the reaction involves either the collision between two diverse particles or two similar particles. For any reaction to take place, the particles must first collide. Whether both the particles are in a gaseous state, or one is solid, and the other is gas, if the pressure is increased, the chances of collision also increase.
When the reactions involve a single particle, things get way complicated as the reactions involve something taking place to a single particle only rather than being generated by the collision between two different particles.
This case works well for the gaseous reactants as they are highly compressible. However, changing pressure for a reaction involving only liquids or solids has no such effect.
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