Ratio of partial pressures of gas

AI Thread Summary
The discussion centers on the relationship between the rate of effusion and the partial pressures of different gas species. It emphasizes that each gas has its own pressure, mass, and effusion rate, while maintaining the same temperature and area. The rate of effusion is directly proportional to the number of molecules, allowing for the calculation of pressure ratios by substituting known values. Participants suggest using the number ratio and masses to derive the pressure ratio effectively. Overall, the conversation highlights the importance of understanding these relationships in gas behavior.
so_gr_lo
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Homework Statement
Bismuth is heated to 1100 K in an oven and gives rise to a beam of vapour molecules effusions from an aperture of area 10^-6 m^2. The beam contains Bi and Bi2 molecules in the ratio 1.41:1. Calculate the ratio of the partial pressures of Bi to Bi2 molecules

I believe the total pressure is the sum of the partial pressures but I’m not sure what to do with that, so I tried just calculating the ratio of the pressures but don’t know where to go from there
Relevant Equations
P=nKT where n is the number density per unit volume

and rate of effusion formula given below
Rate of effusion
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Just guessing here, but try writing your rate of effusion equation for each species separately. Each has its own pressure, mass and effusion rate, but they have the same temperature and area.
 
So this is what I get. since the rate of effusion is proportional to the number of molecules I guess you just plug the given number ratio and masses in and solve for the pressure ratio.

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so_gr_lo said:
So this is what I get. since the rate of effusion is proportional to the number of molecules I guess you just plug the given number ratio and masses in and solve for the pressure ratio.

View attachment 301449
That's what I had in mind, yes. And you know ##N_{B_i}/N_{B_{i2}}, m_{B_i}, m_{B_{i2}}##.
 
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