hi all, I hope to get some help from you. I am getting a headache :mad: from frustration... The question seems so simple but I can not solve :(.
really appreciate if someone can help me. Thanks.

Question) a 0.856g sample of a gaseous compound of sulfur and oxygen exerts a pressure of 644 torr in a 387mL bulb at a temperature of 299K. What is the molar mass of this compound?

ans) 64.1g / mol

hey i got it:
PV=(n/MM)(R)(T)

first convert pressure to atm, 644 torr= 0.85 atm
then plug in and solve for MM
MM=nRT/PV
MM= (.856*.0821*299/.85*.387)
MM=64.1 g

woohoo.

DANG! I got it!! thanks :)

I read this on a post long ago, it might help you...
MW = dRT/P (dirty pee)
:laugh:

I read this on a post long ago, it might help you...
MW = dRT/P (dirty pee)
:laugh:


THANKS!! I will never forget the "massive dirty pee" :laugh::laugh::laugh::laugh:
oh? d= density ???

yes

This is fun to do without a calc!