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What pressure (in ATM) will a sample of O2 gas occupy at 100.0 mL if O2 has a volume of 25.00 mL at 2.0 ATM 4.0 ATM 0.50 ATM 8.00 ATM 2.0 ATM?
Wiki User
∙ 6y ago
First, it helps to look at it backwards. Problems like these are a little overwhelming when you don't know exactly what you're trying to find. So start with density:
D=m/v
Density = mass
Wiki User
∙ 14y ago
Wiki User
∙ 9y agoYou can assume an ideal gas (i.e., use the ideal gas law), and make the simplifying assumption that the temperature does not change. You do need one more piece of information: the final pressure reading. OR. P1v1 = p2v2. , p1 = p2v2/v1. , p1 = p2 15/25= 0.6p2. , 60% of final pressure.
Wiki User
∙ 14y agoFirst, it helps to look at it backwards. Problems like these are a little overwhelming when you don't know exactly what you're trying to find. So start with density:
D=m/v
Density = mass ÷ volume
Now that you know what you need, you figure out what you have. In this case, you don't have density (that's what you're looking for), and you have the mass, so you're looking for volume.
With that mass, we can now find the volume using the ideal gas law. When using the ideal gas equation, n=moles. Therefore, the mass needs to be converted to moles to fit the equation:
Grams ÷ molecular mass = Moles
50.0 grams O2 ÷ 32.0 = 1.56 moles O2
PV=nRT
1.20(v) = 1.56(.0821)300
v = 32.0 L O2
The gas constant is given and remember that temperatures need to be in Kelvin (oC + 273). Now we know both the volume and the mass. Finally, we take the mass and divide it by volume to find density:
50.0 grams ÷ 32.0 L = 1.56 g/L
Wiki User
∙ 12y agoYes and No: it depends on temperature AND amount(moles or grams) in this sample.
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∙ 12y ago227.
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∙ 9y ago1.14
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∙ 6y ago??
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