The temperature has a significant effect on the rate of energy transfer between molecules in a gas-phase reaction. This is because temperature is a measure of the average kinetic energy of the molecules in a system. As the temperature increases, the kinetic energy of the molecules also increases, leading to the following effects:1. Increased collision frequency: As the temperature rises, the molecules move faster, which results in more frequent collisions between them. This increased collision frequency enhances the probability of successful collisions, where molecules have enough energy to overcome the activation energy barrier and react.2. Higher energy collisions: With increased temperature, the energy of the collisions between molecules also increases. This means that a greater proportion of collisions will have enough energy to overcome the activation energy barrier, leading to a higher rate of successful reactions.3. Enhanced molecular orientation: At higher temperatures, the increased molecular motion can lead to better alignment of the reacting molecules, which can further increase the likelihood of successful collisions and reactions.Overall, the rate of energy transfer between molecules in a gas-phase reaction increases with temperature, leading to an increase in the reaction rate. This relationship is often described by the Arrhenius equation, which shows that the reaction rate constant k is proportional to the exponential of the negative activation energy Ea divided by the product of the gas constant R and the temperature T :k = A * e^-Ea / RT where A is the pre-exponential factor, which is a constant specific to the reaction.