Part B The solvent for an organic reaction is prepared by mixing 70.0 mL of acetone (C3H6O) with 64.0 mL of ethyl acetate (C4H8O2). This mixture is stored at 25.0 °C. The vapor pressure and the densities for the two pure components at 25.0 °C are given in the following table. What is the vapor pressure of the stored mixture? Vapor pressure Density Compound (mmHg) (g/mL) 230.0 0.791 95.38 0.900 acetone ethyl acetate Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Psoln: HÅ Units Value ?

The boiling point of chloroform, CHCl3, is 61.700 °C at 1 atmosphere. Kb(chloroform) = 3.67 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.11 grams of the compound were dissolved in 204.7 grams of chloroform, the solution began to boil at 62.577 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? _____g/mol

Calculate the solubility of nitrogen in water at an atmospheric pressure of 0.380 atm (a typical value at high altitude).  Atmospheric Gas Mole Fraction kH mol/(L*atm) N2 7.81 x 10-1 6.70 x 10-4 O2 2.10 x 10-1 1.30 x 10-3 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 x 10-4 3.50 x 10-2 CH4 2.00 x 10-6 1.40 x 10-3 H2 5.00 x 10-7 7.80 x 10-4

A 0.547 g sample of an unknown solute dissolved in 14.0 g of tert-butanol produces a solution with a freezing point of 22.70 °C. What is the molar mass of the solute? For tert-butanol T = 25.50 °C, kf = 9.10 °C · kg · mol-. molar mass = g/mol

Calculate the solubility of nitrogen in water at an atmospheric pressure of 0.500 atm (a typical value at high altitude).  Atmospheric Gas Mole Fraction kH mol/(L*atm) N2 7.81 x 10-1 6.70 x 10-4 O2 2.10 x 10-1 1.30 x 10-3 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 x 10-4 3.50 x 10-2 CH4 2.00 x 10-6 1.40 x 10-3 H2 5.00 x 10-7 7.80 x 10-4      M

Which temperature would allow the highest solubility of CO2 in water? 40C 50C 60C 70C

1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)   2-What is the rate law expression for the reaction A + B → C, based on the following data

sited [Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of diethyl ether, CH3 CH2 OCH2 CH3, is 34.500 °C at 1 atmosphere. K, (diethyl ether) = 2.02 °C/m In a laboratory experiment, students synthesized a new compound and found that when 10.14 grams of the compound were dissolved in 270.0 grams of diethyl ether, the solution began to boil at 34.714 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer ph_08-30-2....pdf Retry Entire Group a a 9 more group attempts remaining C Previous Next 07 Show all 11:14 PM 9/12/2022

the separation of a mixture into pure substance 3. If a solution is made up by mixing 6.0 g of benzoic acid in 1.00 L of water at 42 °C, would the solution be saturated? Would you expect to see solid on the bottom of the container?

At 25.0 °C, the vapor pressure of pure carbon tetrachloride (CCl4) is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr. The molar mass of CHCl3 is 119.38 g/mol and the molar mass for CCl4 is 154.8 g/mol.a. Do you expect the vapor pressure of a pure solvent to differ from the vapor pressure of a solution of that solvent? Why? Use the Raoult’s Law to explain.b. Calculate the vapor pressure in torr of a solution prepared by mixing 25.00 g of CCl4 and 20.00 g of CHCl3. c. Suppose you have a solution which contains CCl4 and CHCl3. Calculate the mole fraction of CHCl3 (XCHCl3) in a solution whose vapor pressure is 185. torr. Please report XCHCl3 with 3 sig figs. Recall the at 25.0 °C, the vapor pressure of pure CCl4 is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr.