start with...
PV = nRT
n = mass / mw
substitute and rearrange...
PV = (mass/mw) RT
mw = mass x RT / (PV)
solve...
mw = (0.481g) x (0.08206 Latm/moleK) x (295K) / ((767torr x 1atm/760torr) x 0.127L)
mw = 90.8 g/mole
Don't kill yourself!
Use PV = nRT, but make sure the P is in atmospheres, the V is in liters and the T is in Kelvins.
(767/760) (0.137 L) = (n) (0.08206) (295 K)
Solve for n, the moles of gas in your sample.
The, divide 0.481 g by the number of moles. That's your answer.
http://www.chemteam.info/GasLaw/Gas-Ideal.html
Be prepared. This is a very popular test question.
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Answers & Comments
Verified answer
start with...
PV = nRT
n = mass / mw
substitute and rearrange...
PV = (mass/mw) RT
mw = mass x RT / (PV)
solve...
mw = (0.481g) x (0.08206 Latm/moleK) x (295K) / ((767torr x 1atm/760torr) x 0.127L)
mw = 90.8 g/mole
Don't kill yourself!
Use PV = nRT, but make sure the P is in atmospheres, the V is in liters and the T is in Kelvins.
(767/760) (0.137 L) = (n) (0.08206) (295 K)
Solve for n, the moles of gas in your sample.
The, divide 0.481 g by the number of moles. That's your answer.
http://www.chemteam.info/GasLaw/Gas-Ideal.html
Be prepared. This is a very popular test question.