Gas Diffusion: HCl & NH3 Reaction Time

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In an experiment on gas diffusion, HCl and NH3 were placed in a glass tube, taking about 5 minutes to meet and form a precipitate despite their mean velocities being around 500 m/s at 25 degrees Celsius. The delay in reaction time is attributed to frequent collisions among HCl molecules, which slows overall movement, similar to a crowded space where individuals bump into each other. The size of the gas molecules also plays a role; HCl molecules are larger and move slower than the lighter NH3 molecules, aligning with Graham's law of diffusion. This highlights the complex dynamics of gas diffusion beyond just molecular speed. Understanding these interactions can provide deeper insights into gas behavior in confined spaces.
erjkism
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i did an experiment involving gas diffusion through a glass tube. HCl was on one side of the tube, while NH3 was on the other side. it took about 5 minutes for the gases to meet in the middle of the tube and form a precipitate.

but the mean velociries of the HCL and NH3 gas molecules at 25 degrees celsius are around 500 m/s. why did it take so long for the molecules to meet and react?
 
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Most of the time the 500m/s HCL molecule is bouncing off other HCL molecules.
Imagine a crowd where everyone is running around in circles bumbing into each other - the crowd as a whole only moves very slowly.
 
k thanks
 
But would not the size of the molecules also effect the transit time. Not being a wise guy, just trying to learn as well. My thinking is the NH3 would be larger, so it would be like cramming a bunch of stuff in a small hole.
 
actually the HCl molecules are larger, and they ended up going quite a bit slower than the lighter NH3 molecules. It goes along with grahams diffusion rate equations
 

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