A mixture containing 33.0 g of an unknown liquid and 230.0 g of water has a freezing point of -1.12 °C. Given kf= 1.86 degree celcius/mol for water, what is the molar mass (g/mol) of the unknown liquid?

The freezing point of benzene, C6H₁, is 5.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in benzene is DDT. A student dissolves 11.78 grams of DDT, C14H9 C15 (354.5 g/mol), in 252.1 grams of benzene. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂ OH CHC13 C6H6 Diethyl ether CH3 CH₂ OCH2 CH3 The molality of the solution is The freezing point of the solution is Kb (°C/m) Kf (°C/m) 1.86 1.99 0.512 1.22 3.67 2.53 2.02 m. °C. 5.12

0.0519 kg of biphenyl (C₁₂H₁₀) is dissolve in benzene (C₆H₆) to create a solution with a total volume of 350.0 mL. (Assume the change in volume is negligible)   What intermolecular forces are shared between biphenyl and benzene? If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL) If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL) What would be the osmotic pressure (in atm) of this solution at 40.0 °C? Assume the density of the solution is the same as benzene, 0.877 g/mL.

1) How many grams of antifreeze (HOCH2CH2OH) would have to be added to 15.0 kg of water in a truck's cooling system to keep it from freezing during a cold Ohio winter with temperatures of -20.0 °C? (Kf for water 1.86 °C/m)

A metal, M, of atomic mass 56 amu reacts with chlorine to form a salt that can be represented as MCly. A boiling point X• elevation experiment is performed to determine the subscript x, and therefore, the formula of the salt. A 34.6 g sample of the salt is dissolved in 100.0 g of water and the boiling point of the solution is found to be 377.34 K. Find the formula of the salt. Assume complete dissociation of the salt in solution. formula:

11. The heat of solution ( Δ Hsoln) is the algebraic sum of the heat of mixing (Δ Hmix), the heat of solvent (Δ Hsolvent) and the heat of solute  (Δ Hsolute).  Which of these four enthalpy changes can only be exothermic?                                  W) Δ Hsoln                   X) Δ Hmix                       Y) Δ Hsolvent                   Z) Δ Hsolute Group of answer choices A.) W B.) Z C.) Y & Z D.) X

How many grams of a hypothetical salt X2Y3 of molar mass 90.00 g/mol would need to be added to 622.00 grams of water to lower the freezing point of water to minus 16.3 degrees C? Use 1.853 degrees C/m for Kf of water. Answer with the unit of g. Your Answer:

Citrus growers protect their fruit from cold temperatures by spraying them with water which releases energy when it freezes. If the grower sprays 375 g of H2O on the fruit tree, how much energy will be released when the water freezes? ΔHfusion of water is 6.01 kJ/mol   dont provide handwritten solution

3. Methanol (CH;OH) has an enthalpy of fusion AHfus = 3.17 kJ/mol and a freezing point of -97.6 °C. Determine the AH associated with freezing 50.0 mL of methanol at -97.6 °C. (The density of methanol is 0.791 g/mL.)

wOn Camp X Dashboard 9Microsoft PowerPoint - Chap X 101 Chem 1 G celsius to kelvin - Goog app.101edu.co Question 6 of 10 A 83.5 g sample of a nonelectrolyte is dissolved in 374.5 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).