ctg202 Posted March 28, 2004 Share Posted March 28, 2004 Can someone please help me with this problem? a gas was found to have a density of 1.13 g L-1 at 22.0 C and a pressure of 755 torr. What is the molecular mass? Link to comment Share on other sites More sharing options...
Kedas Posted March 28, 2004 Share Posted March 28, 2004 Find the amount of molecules based on temperature, pressure (and volume). (Mister Boyle,Charles,Gay-Lussac and Avogadro will help you with that) Then its easy to find the end result. P.S. nice site here to convert the units (if needed): http://www.chemie.fu-berlin.de/chemistry/general/units.html Link to comment Share on other sites More sharing options...
Guest arigordita Posted March 29, 2004 Share Posted March 29, 2004 since theres no correction constant I assume ideal gas law is good enough (e.g. van der walls is not needed): M = dRT/P m = molecular mass d = density R = gas constant (.08206 (l*atm)/(moles*kelvin) t = temperature in K Derived from: P=nRT/V n = m / M (mass divided by Molar mass) P = mRT/VM and m/v = density P = dRT/M MP = dRT M= dRT/P Link to comment Share on other sites More sharing options...
wolfson Posted March 29, 2004 Share Posted March 29, 2004 Yep MW = d x R x T / P is correct. Since no temp was given i would use 273.15K <or> 295K Link to comment Share on other sites More sharing options...
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