Final answer:
Diffusion rates of gases, liquids, and solids differ due to the varying degrees of molecular freedom and interaction. Gases diffuse quickly, following Graham's law, liquids more slowly due to collisions, and solids extremely slowly because of tightly packed molecules. Factors influencing these rates include concentration gradients, molecular mass, surface area, and distance traveled.
Step-by-step explanation:
The relationship between the diffusion rates of solids, liquids, and gases can be explained based on their respective molecular movement and interactions. Gases diffuse relatively quickly because their atoms and molecules move freely and randomly through space, leading to a rapid spread from regions of higher to lower concentration. This process can be described by Graham's law, which states that the rates of diffusion and effusion of gases are inversely proportional to the square roots of their densities or masses.
Liquids have a slower diffusion rate compared to gases because their molecules are in constant motion but have limited space to move before colliding with one another, resulting in a shorter mean free path. Lastly, the diffusion in solids occurs at an extremely slow rate due to the limited movement between tightly packed molecules; as density increases, the diffusion rate decreases even further.
Several factors also affect diffusion rates, including the extent of the concentration gradient, the mass of the diffusing molecules, the amount of surface area available for diffusion, and the distance the molecules must travel. In summary, diffusion rates vary significantly across the different states of matter due to differences in molecular spacing and mobility.