Discover the Distance 2 Gases Meet | Urgent Help Needed!

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To determine the distance at which HBr and NH3 gases meet in a 1.80 m tube, one must apply the kinetic theory of gases, which relates the mean velocity of the gases to their molecular masses. The gases will diffuse toward each other, and the distance each gas travels can be expressed in terms of time. If one gas travels a distance d in time T, the other gas will cover the remaining distance of 1.80 m minus d in the same time. The final calculation will provide the meeting point in centimeters. Understanding these principles will guide the solution to the problem.
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Urgent Help Needed! (gases)

I need some urgent help with figuring out how to find the distance which 2 gases will meet in this question..

Given: Samples of HBr gas and NH_3 gas are placed at opposite ends of a 1.80 m tube.
Question: If the two gases are allowed to diffuse through the tube toward one another, at what distance from each end of the tube will the gases meet and form solid NH_4Br?

Thank you to anyone who can help me with this, or at least set me in the right path.


The distance must be in Cm as well..
 
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One may assume that the gases are at the same temperature.

Apply kinetic theory of gases and determine the mean velocity which is a function of molecular mass.

If one gases travels distance d in time T, then the other must travel 1.8m-d in the same time.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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