Question

Part A Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H, and an unknown amount of propane, C3Hs) were added the same 10.0-L container. At 23.0c C, the total the container is 3.50 atm . Calculate the partial pressure each gas in the container. pressure Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. View Available Hint(s) ΠνΠ ΑΣ Φ atm Previous Answers Submit X Incorrect; Try Again; 5 attempts remaining Part B eous mixture of O2 and N2 contains 30.8 % nitrogen by mass. What is the is 585 mmHg of oxygen in the mixture if the total A pr ess Express you answer numerically in millimeters of mercury. View Available Hint(s) ΠΑΣΦ Poxygen = mmHg

Answer 1

L.atm 1mol |(23 C+273) K 8.00 gx 0.0821 16.04 g K.mol A) Pressure of the the CH4 gas, PH, 10.0 L L.atm (0.499 mol) 0.0821 K.mol296K) 10.0 L 1.21 atm Latm 1mol 18.0 g30.1g |(23 C+273)K K.mol 0.0821 Pressure of the the C2H6 gas, H 10.0 L L.atm (0.598 mol) 0.0821 K.mol(296K) 10.0 L = 1.45 atm + C H C2H Total pressure total Pe 1.21 atm 1.45 atm 3.50 atm Pressure of the the CH gas, P H. = 0.84 atm B) mass percentage of N2 30.8% 69.2% mass percentage of O2 (100-30.8)% 1mol N21.10 mol 30.8 g x No of moles of N, _ 28.02 g 1 mol O2 =2.16 mol 69.2 g x No of moles of O2 32.0 g 2.16 mol 0.6626 Mole fraction of O2, Xo (1.10 2.16) mol N - Partal pressure of the O2 gas, , = (Xo, )Ft 388 mmHg = (0.6626) (585 mmHg) _