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Find the density of O2 at STP conditions and at 3.7 atm?
- Anonymous1 decade agoFavorite Answer
Assume that we have x L of O₂ at STP. Since 1 mole of any gas occupies 22.41L at STP, we have x/22.41 moles of O₂.
Then, since N₂ has a molar mass of 2 * 16 = 32 g/mol, we see that x/22.41 moles of O₂ has a mass of 32 * (x/22.41) = 1.43x grams.
This gives the density of O₂ at STP to be:
Density = Mass/Volume = (1.43x grams)/(x L) = 1.43 g/L.
(Note that the value of x is irrelevant to the density of the gas)
For 3.7 atm, since the pressure and volume of a gas are inversely related, increasing the pressure 3.7-fold will decrease the volume of O₂ by a factor of 1/3.7 = 0.27, we can see that the density will also increase by 3.7-fold. This gives the new density to be 3.7 * 1.43 = 5.29 g/L.
I hope this helps!