CHEM 001 Lecture Notes - Lecture 16: Van Der Waals Equation, Real Gas, Root Mean Square
13 Aug 2020
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Same temperature means different molecules in a mixture have the same average k. e. but, because they have different masses, they have different rms velocities. Setting the two k. e. equal to each other, one can determine the relationship between their rms velocities; more specifically, the ratio. A. molecular weight (directly proportional to effusion rate) D. pressure vs. time graph: effusion rate is the slope. E. graham"s law provides information about two types of gaseous spreading: effusion and diffusion. Definition: spreading of a gas from high pressure to very low pressure through a pinhole, an opening much smaller than the average distances between the gas molecules. B. molecules with higher rms velocities will effuse faster. C. calculated: (effusion rate1/effusion rate2) = sqrt(m2)/sqrt(m1) Definition: the spreading of one gas into another gas or into empty space. B. diffusion rate is much slower than rms velocity because gas molecules collide with each other as they diffuse. C. calculated: (diffusion rate1/diffusion rate2) = sqrt(m2)/sqrt(m1)
