Question

A 10.0L. tank at 1.79 C is filled with 18.8 g of chlorine pentafluoride gas and 7.10 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction chlorine pentafiuoride afm partial pressure: mole fraction: carbon diaxide atm partial pressure atm Total pressure in tank

Answer 1

V = 10 lit T=1.796 - 1.79 + 273:15 T- 274.94K Chorine penta fluonicle (cifs) = 18.8gm MM = 35.45 +5(19) = 130:45 naifs = 78.8 mol = 0.14411652 mol 130.45 Carbon dioxide (CO2) = 7.10 gm MM = 44.01 gmimo nco = 7:| 0.161326971 mol 04.01 mole fraction (x) X CIFs = nelfs & Olun Oly4 + Oʻ16) Cify + n cos [Xcifs = 0.472 Ane Xco, = 1- XCIFS 7 1-0.472 (xcą = 0.528/dome

Partial pressure neifs XRT O JUU x 0.0821 x 274-94 10 Palfs = Polfs = 0.325 atm Pcos - "coz XRI > 0.16) *0.0821 Y 274.94 10 Pcqz = 0.36 3 atm one