How does increasing pressure affect the reaction rate of gases?

How does increasing pressure affect the reaction rate of gases?

• A. It decreases the chance of particle collisions
• B. It can increase the rate by increasing collision frequency
• C. It has no effect on gas reactions
• D. It lowers the temperature of the reaction

Answer: (B)

Increasing pressure in a system containing gases leads to a higher concentration of gas particles in a given volume. When pressure is increased, the gas molecules are pushed closer together, which significantly increases the frequency of collisions between them. Since reaction rates are dependent on the frequency of effective collisions between reactant molecules, a higher collision frequency directly correlates with an increased rate of reaction. This phenomenon aligns with the principles of collision theory, which states that for a reaction to occur, particles must collide with sufficient energy and proper orientation. Thus, the correct understanding is that increasing pressure enhances the likelihood of these effective collisions, resulting in a faster chemical reaction rate.

Increasing pressure in a system containing gases leads to a higher concentration of gas particles in a given volume. When pressure is increased, the gas molecules are pushed closer together, which significantly increases the frequency of collisions between them. Since reaction rates are dependent on the frequency of effective collisions between reactant molecules, a higher collision frequency directly correlates with an increased rate of reaction. This phenomenon aligns with the principles of collision theory, which states that for a reaction to occur, particles must collide with sufficient energy and proper orientation. Thus, the correct understanding is that increasing pressure enhances the likelihood of these effective collisions, resulting in a faster chemical reaction rate.