1. Calculate the mass of oxygen (in mg) dissolved in a 6.00 L bucked of water ex
ID: 994627 • Letter: 1
Question
1. Calculate the mass of oxygen (in mg) dissolved in a 6.00 L bucked of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.32 and the Henry’s law constant for oxygen in water at this temperature to be 1.7 X 10-3 M/atm.
2. At a given temperature the vapor pressures of benzene and toluene are 145 mm Hg and 60.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0.650.
3. Calculate the freezing point of a solution of 800.0 g of ethylene glycol (C2H6O2) dissolved in 400.0 g of water. Kf= 3.14C/m and Kb= 0.321C/m
Explanation / Answer
1.
M = H*Pi
M = 1.7*10^-3)(0.32)
M = 0.000544 mol of O2 per liter
V = 6 L so
mol = MV = 0.000544*6 = 0.003264 mol of oxygen
mass = mol*Mw = 0.003264*32 = 0.104448 g of O2 = 104.45 mg of O2
NOTE Consider posting multiple questions in mutliple set of Q&A.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.