You can first calculate the total moles of gas at 100 atm using PV = nRT. The problem states that if this gas mixture is used at 1.00 atm (760 torr) pressure, the partial pressure of methoxyflurane is 1.2 torr. Thus the fraction 1.2 torr / 760 torr will be the equivalent to the mole fraction of methoxyflurane also since pressures are directly proportional to moles. This is also the mole fraction of methoxyflurane in the original 100 atm mixture, so just multiply the total moles by 1.2 / 760 to get the moles of methoxyflurane, and convert to grams. That should do it!
The original question got deleted somehow; here it is again for reference:
"How many grams of methoxyflurane (C3H4Cl2F2O) must be present in a 49.0 L tank of compressed air with a pressure of 100. atm at 25.0°C in order for 1.2 mm Hg pressure of methoxyflurane to be present in the lungs of a patient at 1.00 atm?"
Interesting compound and subject - here's an article about it.
Steve
http://www.medicaldev.com/MEOF_Paper.pdf: "Methoxyflurane (MEOF) is the only volatile anaesthetic with significant analgesic properties1. It has a long history of use to relieve pain with minimal sedative effects."
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