Final answer:
The statement 'Higher temperature => faster particles (more KE)' indicates that increasing temperature results in greater kinetic energy and speed of particles, facilitating more frequent and energetic collisions that can lead to chemical reactions.
Step-by-step explanation:
Higher temperature results in faster-moving particles, as it increases the kinetic energy (KE) of these particles. At increased temperatures, particles gain more thermal energy, which translates into greater motion, leading them to collide more frequently and with greater energy, making chemical reactions more likely to occur.
For instance, when temperature rises, gases composed of lighter molecules exhibit more high-speed particles and a higher root mean square speed (Urms). Conversely, heavier molecules have more low-speed particles and a lower Urms. Thus, the average kinetic energy of the particles is heightened with a rise in temperature, which not only causes more collisions but also increases the probability of overcoming the reaction's activation energy barrier.
In summary, the statement Higher temperature => faster particles (more KE) emphasizes the direct relationship between temperature and the kinetic energy - and therefore the speed - of particles in a substance.