Assume that each of the substances below costs the same amount per kilogram. Which would be the most cost-effective to use to lower the freezing point of water? Explain. (i) KCI (ii) NaCI (ii) MgCl2 Atomic masses (g/mol): Na =23.0; Mg = 24.3; Cl = 35.5; K = 39.1 %3D

The vapor pressure of chloroform is 173.11 mm Hg at 25°C.How many grams of cholesterol, C27H46O, a nonvolatile, nonelectrolyte (MW = 386.6 g/mol), must be added to 280.3 grams of chloroform to reduce the vapor pressure to 169.22 mm Hg ?chloroform = CHCl3 = 119.40 g/mol. g cholesterol

The normal boiling point of a certain liquid X is 128.10 °C, but when 35.3 g of urea (CH4N2O) are dissolved in 350. g of X the solution boils at 130.9 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. °C-kg ☐ x10 K-0 = mol 5

(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. CaCl₂(s) Cal₂(s) Lattice Energy -2247 kJ/mol -2059 kJ/mol * Explain. ΔΗ soln -46 kJ/mol -104 kJ/mol *Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s). calcium chloride 2201 calcium iodide 1955 XkJ/mol X kJ/mol (b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water? chloride iodide The enthalpy of hydration for CaCl₂ is more exothermic than for Cal2. Any differences must be due to differences in hydrations between CI and I¯.

(d) Determine the freezing point and boiling point of the solution. (Assume density of water = 1.00 g/mL; Kf= 1.86oC/m; Kb= 0.512oC/m; density of EG = 1.114 g/mL

In order to freeze ice cream, the freezing point of water must be reduced from 0.0 C to –8.0 C.  How many grams of salt (NaCl) are required to lower the freezing point of 250 mL of water this much?

The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25°C. How many grams of aspirin, C9HsO4, a nonvolatile, nonelectrolyte (MW = 180.1 g/mol), must be added to 218.9 grams of diethyl ether to reduce the vapor pressure to 456.11 mm Hg? diethyl ether = CH3CH₂OCH₂CH3 = 74.12 g/mol. Mass= Submit Answer Retry Entire Group No more group attempts remain

Calculate the vapor pressure of a solution of 23.5 g of glycerol (C₂H₂O3) in 500.0 g of water at 25.0 °C. The vapor pressure of water at 25.0 °C is 23.76 torr. (Assume ideal behavior.) Be sure your answer has the correct number of significant figures. torr ☐x10 X

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