p1=Y1 PTotal and p2 Y2 Ptotal In any mixture of IDEAL gases the partial pressure of each gas in the mixture is defined by its MOLE FRACTION and the TOTAL PRESSURE 12 PDF文件使用"pdfFactory Pro”试用版本创建鳍m,fineprint.com,cn
12 p1 = Y1 PTotal and p2 = Y2 Ptotal In any mixture of IDEAL gases the partial pressure of each gas in the mixture is defined by its MOLE FRACTION and the TOTAL PRESSURE PDF 文件使用 "pdfFactory Pro" 试用版本创建 嘀www.fineprint.com.cn
EXAMPLE: A Mixture of He and O,is used in scuba diving tanks. If for a particular dive 46 L of O,at 25C (1 atm)and 12 L of He at 25C (1 atm)were pumped into a 5 L tank what would be the partial pressure of each gas and the total tank pressure at 25C? Calculate the number of mole of each gas n(0)=PV1RT=(1.0x46)/0.0821x298)mol=1.9mol n(He)=PV/RT=(1.0x12)/(0.0821x298)mol=0.49mol Now V=5.0 L The partial pressures of each gas is therefore p(02)=nRTW=(1.9x0.0821x298)/5.0atm=9.3atm p(He)=nRTW=(0.49x0.0821x298)/5.0atm=2.4atm TOTAL PRESSURE =(9.3+2.4)atm =11.7atm(1185kPa) (Note:1 atm 101.3 kPa) 13 PDF文件使用"pdfFactory Pro”试用版本创建暗m,fineprint..com,cn
13 EXAMPLE: Calculate the number of mole of each gas n (O2 ) = PV/RT = (1.0 x 46)/(0.0821 x 298)mol = 1.9 mol n (He) = PV/RT = (1.0 x 12)/(0.0821 x 298) mol = 0.49 mol Now V = 5.0 L The partial pressures of each gas is therefore p(O2 ) = nRT/V = (1.9 x 0.0821 x 298)/5.0 atm = 9.3 atm p(He) = nRT/V = (0.49 x 0.0821 x 298)/5.0atm = 2.4 atm TOTAL PRESSURE = ( 9.3 + 2.4)atm = 11.7 atm (1185 kPa) (Note: 1 atm = 101.3 kPa) A Mixture of He and O2 is used in scuba diving tanks. If for a particular dive 46 L of O2 at 25oC (1 atm) and 12 L of He at 25oC (1 atm) were pumped into a 5 L tank what would be the partial pressure of each gas and the total tank pressure at 25oC? PDF 文件使用 "pdfFactory Pro" 试用版本创建 嘀www.fineprint.com.cn