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100g O2 = 3.125 mol O2 (since 1 mol O2 = 32 g) 25 degrees C = 298 K 1.50 atm remains 1.50 atm Gas constant when dealing with pressure in atm is 0.082 Plug these values into the equation: PV=nRT 1.50 atm x V = 3.125 mol x 0.082 x 298 K V = 50.9 FINAL ANSWER: 50.9 L
Wiki User
∙ 11y ago
Wiki User
∙ 12y agoUse the general 'Ideal Gas' law:
p.V = n.R.Tor
V = n.R.T/pp=pressure in atm (atmosphere)
V=volume in Litres
n= number of moles
T=absolute temperature in K (= oC + 273)
and R is the general 'gas constant' = 8.02*10-2 L.atm.K-1.mol-1
Or in Standard international units (SI-units):
p=pressure in Pa (pascal)
V=volume in m3
n= number of moles
T=absolute temperature in K (= oC + 273)
and R is the general 'gas constant' = 8.31 J.K-1.mol-1
This is valid for ANY kind of (ideal) gas (at about normal or low temperature, normal or lower pressure; all of the given values are OK)
Wiki User
∙ 14y agoUse the ideal gas law:
PV=nRT
Pressure(volume) = moles(gas constant)Temperature
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
143.6 grams O2 ÷ 32.0 grams = 4.49 moles O2
.450(v) = 4.49(.0821)356
v = 292 L O2
The gas constant is given and remember that temperatures need to be in Kelvin (oC + 273).
Wiki User
∙ 14y agouselah the formula from the book . dont be lazy lah .you have much more time
Wiki User
∙ 11y agoAny volume you like - it depends on the quantity of O2 you have!
Wiki User
∙ 6y agoThe volume is 70 L.
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