When a bottle of perfume is opened, odorous molecules mix with air and slowly diffuse throughout the entire room. Is ΔG for the diffusion process positive, negative, or zero? What about ΔH and ΔS for the diffusion?

Verified step by step guidance

1. Step 1: Understand the concept of diffusion. Diffusion is the process by which molecules spread from an area of high concentration to an area of low concentration, resulting in a more uniform distribution of molecules.
2. Step 2: Consider the change in Gibbs free energy (ΔG) for the diffusion process. Since diffusion is a spontaneous process, ΔG is negative. Spontaneous processes occur without the input of external energy and result in an increase in entropy.
3. Step 3: Analyze the change in entropy (ΔS) for the diffusion process. As the perfume molecules spread throughout the room, the disorder or randomness of the system increases. Therefore, ΔS is positive.
4. Step 4: Evaluate the change in enthalpy (ΔH) for the diffusion process. Diffusion is typically an isothermal process, meaning it occurs at constant temperature without a significant change in heat content. Thus, ΔH is approximately zero.
5. Step 5: Summarize the thermodynamic changes: For the diffusion of perfume molecules, ΔG is negative (spontaneous process), ΔS is positive (increase in disorder), and ΔH is approximately zero (isothermal process).