' x ' g of molecular oxygen O 2 is mixed with 200 g of neon Ne . The total pressure of the nonreactive mixture of O 2 and Ne in the cylinder is 25 bar. The partial pressure of Ne is 20 bar at the same temperature and volume. The value of ' x ' is [Given: Molar mass of O 2 = 32 g mol - 1 . Molar mass of Ne = 20 g mol - 1 ]

Step-by-step solution

Given O 2 + Ne Xgm   200 gm P total = 25 bar; P Ne = 20 According to Dalton's law of partial pressure. P O 2 + P Ne = 25 P O 2 = 25 - 20 = 5 bar Also, P O 2   =   X O 2 P T         Where   X O 2 =   mole   fraction   of   oxygen   gas . 5 = x 32 x 32 + 200 20 × 25 5 x = x + 320 4 x = 320 x = 320 4 = 80 gm