In chemistry, you hear people mention “at STP”.\u00a0 STP means standard temperature and pressure<\/strong>.\u00a0 Standard pressure is 1 atmosphere; standard temperature, curiously, is 0\u00b0C.<\/p>\n The relevance of standard temperature and pressure is that, at those particular settings, the volume of an ideal gas is 22.4L\/mole.\u00a0 Note that the molar volume is independent of the molar mass of the gas, so long as it closely follows the “ideal gas” concept.\u00a0 Mortimer reports that, at STP, most gases closely follow ideal behaviour.<\/p>\n Example:\u00a0 Find the volume of 1.000 kg of CO2<\/sub> at STP.<\/strong><\/p>\n Solution: We must first convert the mass to moles (see my post here<\/a> and perhaps even here<\/a> for more about that), as follows (M.M. meaning molar mass):<\/p>\n From the periodic table of the elements, M.M. of CO2<\/sub>=12.0g+2(16.0g)=44.0g<\/p>\n We proceed with our conversion from kilograms to L, using the factor 22.4L\/mol:<\/p>\n 1) 1.000kg=1000.g<\/p>\n 2) 1000.g x 1mol CO2<\/sub>\/44.0g = 22.7273mol CO2<\/sub><\/p>\n 3) 22.7273mol CO2<\/sub> x 22.4L\/mol = 509L CO2<\/sub><\/p>\n The one-line chemistry method you might see on the board combines the steps:<\/p>\n 1.000kg x 1000.g\/kg x 1mol CO2<\/sub>\/44.0g x 22.4L\/mol = 509L CO2<\/sub><\/p>\n Apparently, based on the molar volume of 22.4L\/mol, 1.000kg of CO2<\/sub> has volume 509L at STP (1 atmosphere and 0\u00b0C).<\/p>\n There is much more to say about volumes of gases. I’ll be talking more about them in future posts.<\/p>\n HTH:)<\/p>\n Source:<\/p>\n Mortimer, Charles E. Chemistry<\/em>, 6th Ed. Belmont: Wadsworth, 1986.<\/p>\n