How does the pressure affect the rate of reaction?

Answer 1

The concentration of reactants is changed.

If the reaction occurs in the gas phase

Answer 2

Increasing the pressure on a reaction involving reacting gases increases the rate of reaction if in a balanced chemical equation number of moles of products are less than reactants,as

N2 + 3H2 ------>2NH3

But if number of moles of products are higher than reactants then the increase in pressure decreases the rate of reaction,as

2SO3----->2SO2 + O2

AND,

The change of pressure does not effect those gaseous reactions in which number of moles of products and reactants are the same as,

H2 + Cl2 ----> 2HCl

Answer 3

Pressure will speed up a chemical reaction.

The reason for this is that pressure reduces the space between the molecules in a reaction. This means that the molecules will collide more often, which gives them more opportunity to react with each other.

Answer 4

It depends very much on the moles of gasses present i.e. (Sorry, I can't find an equilibrium arrow)

2[A](g) + B(g) -----> 2[C](g) + [D](l)

On the left hand side there is 3 mols of gas, compared with the right hand side where there is 2 mols of gas, so if the pressure was increased it would shift to the right to reduce the effects of the change, while if the pressure was decreased it would shift to the left.

However if the equation were to be like this

2[A](g) + B(l) -----> 2[C](g) + [D](l)

Pressure would not effect it as there is two mols of gas on the right and two mols of gas on the left so neither side of the equilibrium would help reduce the effect of the change.

Answer 5

The more pressure, you have, the faster the reactions. This is because in a more tightly packed place, there will be more collisions.

For Example, if I had a large container and small container which container the same number of particles in each container, which container would have a faster reaction?

The answer is the small container because, since there is smaller space ( which means there is more pressure), the particles are more likely to bounce off the walls of the container and collide. Thus, the more collision's, the faster the reaction.

I hope this helped :)

Answer 6

It only affects the rate of chemical reactions if gases are involved in the reaction. And the it depends on how many moles of gas are present on the reactant and the product side of the reaction. If you have a specific example, post that and we can answer it better.

Answer 7

Increasing pressure typically increases the rate of reaction for gas-phase reactions by bringing gas molecules closer together and increasing the frequency of collisions, which leads to more successful collisions. However, for reactions involving only solids or liquids, pressure usually has little to no effect on the rate of reaction.

Answer 8

If the pressure increase the number of intermolecular collisions increase and so the reaction rate. This is valid for gases.

Answer 9

gravity