Part A: Volume of Cyclohexane mL Mass of cyclohexane (d= 0.7786 g/mL) 6.0 Freezing Point of cyclohexane °C 128 Part B: Molecular Weight of Naphthalene g/mol 0.23 Mass of Sample 1 Moles of Sample 1 Mass of Sample 2 0.18 Moles of Sample 2 m (mol/kg solvent) T,('C) AT, Moles Naphthalene 5.1 TRIAL 1 - 5.3 TRAIL 2 CC/m) 1 Cuelehexane

Solution freezing point

3) Calculate the freezing point (oC) of a solution of 15.46 g of acetone (CH3COCH3, MM = 58.08 g/mol) in 85.0 g of CCl4, whose normal freezing point is –23.0 oC. ​ Given: P = 1 atm​​Kf CCl4 = 29.8 oC/m a) –55.6 ​ b) –93.3​ c) 35.7​ d) –76.4 ​e) 70.3​​ f) –116

Given the following mixture of two compounds 70.00 mL of X (MW =80.00 g/mol)(density 0.800 g/mL) and 820.00 mL of Y (73.00 g/mol))(density 1.056 g/mL). The freezing point of pure Y is 17.00 degrees C. The molal freezing constant is 3.091 degrees C/m. What is the freezing point of the solution, in degrees C?

In an aqueous solution of sulfuric acid, the concentration is 7.21 mol% of acid. The density of the solution is 1.2033 g mL-1. Calculate the molal concentration of the H2SO4. Molality = i m H2SO4 Calculate the mass percent of the acid. % (w/w) H2SO4 Calculate the molarity of the solution. Molarity = MH2SO4

Moving to another question Wll tion 10 Calculate the molality of C2H5OH (molar mass = 46.068 g mol-1) in a water solution that is prepared by mixing 40.17 g of C2H5OH with 441.6 mL of H2U at 20 °C. (Density of water 1.00 g mL) (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) K Question 10 of 29 A Moving to another question will save this response. 211 * LO, %23 24 & 2. 3 8 delete 4 E R Y [O P ente S D F G K L. ret C- V alt alt option n command command option

A bottle on the stockroom shelf reads 41% sodium hydroxide solution. What is the molality of this solution? Recall that the % means (w/w) percentage. molality = m NaOH eTextbook and Media Save for Later Attempts: 0 of 15 used Submit A O S MacBook Air

What is the molality of a4.60%v/vsolution of isopropanol. The density of water is0.9978 g/mLand the density of isopropanol is0.786 g/mL. The molar mass of water is18.02 g/moland the molecular mass of isopropanol is60.1 g/mol.  ( please type answer not write by hend )

10:16 S 57% Question 11 of 15 0/2 POINTS EARNED A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of 12 benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. What was the molality of the solution? a O of 0.67 points earned L 3 attempts remaining How many moles of the unknown compound were dissolved in the b solution? L 0 of 0.67 points earned 3 attempts remaining What is the molar mass of the unknown compound? L O of 0.67 points earned 3 attempts remaining II

Please find the following with the information provided in the pictures: -freezing point of solvent - freezing point of solution - depression of freezing point - molecular weight of the unknown - determine molality - determine moles of solute - determine molecular weight weight of solvent is: 25.004g weight of solute is: 4.502g