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Molar concentrations and partial pressures?
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2 Responses to Molar concentrations and partial pressures?
Why not? … Sounds great!
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Divide each mass by their molar weight to get the number of moles of each gas. 0.856g He/(4.003 g He/mole) = 0.214 mole of He. Do that for all the masses and add them up. I got a total of 1.034 moles.
From that you could find the total pressure using PV=nRT.
Next, find the mole fraction (I think this is the same as molar concentration) which is the # of moles of each gas/total number of moles.
Then multiply each mole fraction by the total pressure to get each partial pressure.
Hope this helped. Let me know if you want me to go through each step.
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