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Title: How to calculate the rate of diffusion based on different level of concentration? Post by: oemBiology on Sep 15, 2022 Diffusion: movement of solute molecules from an area of higher concentration to an area of lower concentration
Referring to following link, I would like to know on whether calculation is correct or not for calculating the rate of diffusion. (https://biology-forums.com/gallery/45/94679_15_09_22_7_56_18.png) (https://biology-forums.com/index.php?action=gallery;sa=view&id=45378) (https://biology-forums.com/gallery/45/94679_15_09_22_8_15_03.png) (https://biology-forums.com/index.php?action=gallery;sa=view&id=45379) J = [D x A x (C1 - C2)] / L Case 1 (C1 - C2) = 10 C1 = 400 C2 = 390 Case 2 (C1 - C2) = 10 C1 = 40 C2 = 30 Would both cases be the same speed in term of rate of diffusion? Does anyone have any suggestions? Thanks in advance https://www.youtube.com/watch?v=JgAKv1Zlgcw Title: Re: How to calculate the rate of diffusion based on different level of concentration? Post by: duddy on Oct 15, 2022 For a gas, the rate at which diffusion occurs is proportional to the square root of the density of the gas. The density of a gas is equal to the mass of the gas divided by the volume of the gas. If the volume is held constant one gas is compared with another with another,
\(\frac{R_2}{R_1}=\sqrt{\frac{M_1}{M_2}}\) where R is the rate of diffusion in mol/s and M is the molar mass in g/mol. This is known as Graham's law of diffusion. So if you want to answer your question, plug-in different values into this formula to see what happens. For example: Compare the rate of diffusion between fluorine and chlorine gases. Fluorine gas, F2, has a molecular mass of 32 grams. Chlorine gas, Cl2, has a molecular mass of 70.90 grams. \(\frac{R_2}{R_1}=\sqrt{\frac{_{70.9\ g}}{32\ g}}=1.49\) Therefore, fluorine gas is 1.49 times as fast as chlorine gas. |