Question

9. Chlroform and ether were common anesthetic agents in the late 1800s as delivered as a vapor. A novice physician in the 1800s thought it would be a good idea to mix the two agents. At a certain temperature the vapor pressure of pure diethyl ether (C4H100) is measured to be 0.7 atm. Suppose a solution is prepared by mixing 50.0 g of diethyl ether and 50,0 g of chloroform (CHCl3). Calculate the partial pressure of diethyl ether vapor above this solution. You may assume the solution is ideal. Molar mass C4H100 = 74.1216 g/mol Molar mass CHCl3 = 119.37764 g/mol A. B. C. D. E 0.3 atm 0.4 atm 0.5 atm 1.8 atm 0.7 atm

Answer 1

Ansig PE = 0.7 atin mass of ether= 50g , mW of ether = 74.1216 Moles of ether= Mas 50% Molarmas 74.1216 gmolt Moles of ethor, ne = 0.6746 mol MW of ChUz = 119.377 dugnał mass of chloroform, = 50g, = 50 g Moles of CH4 = n 119:37964 g mol' Me=0.419 mol Partial pressure of, Pe= PEXE diethyl ether above miniture of solution PE=P Exne ne the X® - W8-4 Ba Cuen of ether 2007 atin x 0.6746 mol (0-6746 +0-419) mol = 0.7 atm x 0.676 1.0936 PE= 0.432 atm option (B) is wrrect. So