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Unformatted text preview: R Units Value L atm/mol K 0.08206 cal/mol K 1.987 J/mol K 8.314 m 3 Pa/mol K 8.314 L torr/mol K 62.36 Example: If we had 1.0 mol of gas at 1.0 atm of pressure at 0°C (273.15 K), what would be the volume? PV = nRT V = nRT/P V = (1.0 mol)(0.0821 L atm/mol K)(273 K)/(1.0 atm) V = 22.41 L • 0 °C and 1 atm pressure are referred to as the standard temperature and pressure (STP) The molar volume of an ideal gas (any ideal gas) is 22.4 liters at STP Example: Nitrate salts (NO 3) when heated can produce nitrites (NO 2) plus oxygen (O 2 ). A sample of potassium nitrate is heated and the O 2 gas produced is collected in a 750 ml flask. The pressure of the gas in the flask is 2.8 atmospheres and the temperature is recorded to be 53.6 °C. How many moles of O 2 gas were produced? PV = nRT n = PV/RT n = (2.8 atm * 0.75 L) / (0.0821 L atm/mol K * (53.6 + 273)K n = (2.1 atm L) / (26.81 L atm/mol) n = 0.078 mol O 2 were produced...
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 Fall '10
 LauraChoudry
 Chemistry, pH, idealgas equation

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