What effect does increasing pressure have on reacting gases?

Increasing pressure in a system involving reacting gases typically leads to an increase in the reaction rate. This occurs because increasing the pressure effectively reduces the volume available for the gas molecules. When the volume decreases, the gas molecules become closer together, which increases the frequency of collisions between them.

More collisions per unit time enhance the likelihood that reactant molecules will interact, leading to more successful reactions occurring. According to the collision theory of chemical reactions, the rate of reaction is dependent on the frequency of successful collisions between reactant particles. Therefore, by elevating the pressure, the chances of these collisions occurring increase, resulting in a higher reaction rate.

The alternative options do not account for the relationship between pressure and collision frequency in the context of reacting gases.