Why does increasing the pressure of a gas usually increase reaction rate?

a. the increased pressure acts as a catalyst on the gas particles in the reaction.

b. the gas particles are closer, which increases the number of collisions.

c. the speed of the gas particles increases, which increases the number of collisions.

d. the surface area of the gas particles increases, which increases the number of collisions.

Option (B) is the correct answer.

Explanation:

According to collision theory, rate of a reaction generally increases when there is increase the surface area of reactants, more number of collisions between the particles etc.

Since, it is known that gas molecules have high kinetic energy. So, when pressure is applied on a gas then its particles come closer to each other. As a result, there will be increase in number of collisions between the particles.

Hence, the rate of reaction will increase will more number of collisions between the particles.

Thus, we can conclude that increasing the pressure of a gas usually increase reaction rate because the gas particles are closer, which increases the number of collisions.

fdvwsa gfwsargebgeebbfwfwffw gwf   vgwgw gw f gwgw fgw v v dsv dwfff

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.