A certain substance X condenses at a temperature of 108.9°C. But if a  950.g sample of X is prepared with 105.5g of urea ((NH2)2CO) dissolved in it, the sample is found to have a condensation point of 112.2°C instead. Calculate the molal boiling point elevation constant  Kb of X. Round your answer to 2 significant digits

A solution of ethanol (CH,CH,OH) and water that is 90.% ethanol by mass is boiling at 81.9 °C. The vapor is collected and cooled until it condenses to form a new solution. Calculate the percent by mass of ethanol in the new solution. Here's some data you may need: normal vapor pressure density boiling point at 81.9 °C g 0.79 mL ethanol 78. °C 865. torr 100. °C 1.00 mL 389. torr water Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution and vapor above it are ideal. ?

Part H Calculate the boiling point for 0.41 mol ethylene glycol and 0.18 mol KBr in 128 g H₂O. Express your answer in degrees Celsius to one decimal place. [5] ΑΣΦ bp = S ? °C

How many grams of sucrose (C₁2H₂2011) must be added to 669 g of water to give a solution with a vapor pressure 0.981 mmHg less than that of pure water at 20 °C? Be sure your answer has the correct number of significant digits. Note: Reference the vapor pressure of water (H₂O) at selected temperatures table for additional information. C12H22011 x10 X

At 25.0 °C the Henry's Law constant for nitrogen monoxide (NO) gas in water is 0.0019 M/atm. Calculate the mass in grams of NO gas that can be dissolved in 1200. mL of water at 25.0 °C and a NO partial pressure of 1.47 atm. Be sure your answer has the correct number of significant digits. 08 x10 X S

The normal boiling point of a certain liquid X is 131.10°C, but when 32.9g of glycine (C2H5NO2) are dissolved in 600.g of X the solution boils at 132.1°C instead. Use this information to calculate the molal boiling point elevation constant Kb of X.Round your answer to 2 significant digits. Please do not round untill the end =Kb⋅°Ckgmol

At 25.0 °C the Henry's Law constant for hydrogen sulfide (H, S) gas in water is 0.087M/atm. Calculate the mass in grams of H, S gas that can be dissolved in 1325. mL of water at 25.0 °C and a H, S partial pressure of 1.58 atm. Be sure your answer has the correct number of significant digits. x10

With the given data, calculate the enthalpy of hydration for both lithium chloride (LiCl) and sodium chloride (NaCl). Which of the two cations, lithium or sodium, will establish the strongest ion-dipole interactions with water? Explain. Lithium chloride has a lattice energy of -834kJ/mol and ΔHsol = -37,0 kJ/mol sodium chloride has a lattice energy of -769kJ/mol and ΔHsol = +3,88 kJ/mol.

At a certain temperature the vapor pressure of pure benzene (C6H6) is measured to be 0.68 atm. Suppose a solution is prepared by mixing 88.0 g of benzene and 64.1 g of thiophene (C4H4S). Calculate the partial pressure of benzene vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal. 0 atm 0x10 X

A certain liquid X has a normal freezing point of 4.10 °C and a freezing point depression constant K,=2.77 °C-kg-mol¯¹. Calculate the freezing point of a solution made of 40.g of sodium chloride (NaCl) dissolved in 800. g of X. Round your answer to 1 significant digit. [°C x10 X Ś