• This is the process by which different gases or different liquids mix and is due to the random motion of their particles
• Diffusing particles move from an area of?high concentration?to an area of?low concentration
• Eventually the concentration of particles is?even?as they spread out to occupy all of the available space
• Diffusion happens on its own and no energy input is required although it occurs faster at higher temperatures

Diffusion of potassium manganate(VII), KMnO_4?,?in water. After a few hours the concentration of KMnO_4?is the same throughout the solution

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• Diffusion occurs much?faster?in gases than in liquids as gaseous particles move much quicker than liquid particles
• At the same temperature, different gases do not diffuse at the same rate.
• This is due to the difference in their?relative molecular masses
• Lighter gas particles can travel faster and hence further, therefore the lower its relative mass the faster a gas will diffuse
• This can be demonstrated in the reaction between ammonia, NH₃, and hydrogen chloride gas, HCl, inside a long glass tube
• Where the two gases meet a white smoke of ammonium chloride, NH₄Cl, is formed
• This does not occur in the middle of the tube as you might expect, but much closer to the end with the hydrogen chloride (M_r?= 36.5) and the ammonia (M_r?= 17) molecules are smaller and lighter

NH₃?molecules have less mass than the HCl molecule, so diffuse faster, hence the product (a white smoke of NH₄Cl) forms closer to the end where the HCl is

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