Thermodynamics and Gas expansion

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The discussion focuses on a thought experiment involving the diffusion of laughing gas (N2O) and tear gas in a classroom setting. Participants explore how to determine which row of students will first experience both gases, emphasizing the importance of molecular mass and diffusion rates. The kinetic energy formula is mentioned, but the lack of specified temperature raises questions about assumptions for calculations. It is suggested that assuming a uniform room temperature is reasonable for determining the diffusion fronts. The key takeaway is that relative thermal speeds of the gases will dictate where the two gases meet.
InfernalAsylum
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Here's the Question:
In a Classroom there are 50 rows of students. A container of N20 (laughing gas) was opened at the front row and tear gas (molar mass 240 gm/mole) was opened simultaneously at the rear of the room. Which row of students will be the first to be laughing with tears in their eyes? mm(N)=14 & mm(O)=16
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I thought I could solve it by using KE=3/2 KT and then after finding out the kinetic energy... substitute and solve for Velocity in KE=1/2 mv²
However.. in the problem it doesn't say anything about the temperature in the room so I don't know if i should assume that it's room temperature or if there's another way to solve this... Any help is appreciated.
 
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I think it's safe to assume the temperature is uniform throughout the room. You only need the relative thermal speeds of the molecules to determine where the two "diffusion fronts" will meet.
 
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