Molar mass An unknown gas occupies a volume of 1.50L at 21 degrees C and 0.950 atm. If the mass is 2.01g what?

PV = nRT

n = mass / mw

substitute and rearrange...

PV = (mass / mw) RT

mw = mass RT / (PV)

solving..

mw = (2.01g) x (0.08206 Latm/moleK) x (294.15K) / ((0.950 atm) x (1.50L)) = 34.0 g/mole

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looks like you did this

2.01 x 0.08206 x 294.15 x 0.950 / 1.50

instead of this

2.01 x 0.08206 x 294.15 / 0.950 / 1.50

see the difference?

appropriate gasoline regulation: P*V = n*R*T sparkling up for n, the kind of moles: n = P*V/(R*T) on condition that all of us recognize the mass and the formula for moles, divide as such to get molar mass: M = m/n therefore: M = m*R*T/(P*V) files: m:=2.01 grams; R:=0.08205 L-atm/mole-ok; T:=294.15 ok; V:=a million.50 Liters; P:=0.950 atm; effect: M = 34.04 grams/mole My wager is that the gasoline flavor is hydrogen peroxide.

use ideal gas equation,

PV=nRT