When 9.730 g of aspirin was dissolved in 102.7 g of benzene, the freezing point was 275.9 K. What is the formula mass of this compound? The freezing point depression constant for benzene is 5.12 (°C*kg)/mol. The melting point and boiling points are 5.50°C and 80.10°C, respectively.

M 2req 2req M M Visited Use the References to access important values if needed for this question. The boiling point of ethanol CH3 CH₂OH is 78.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is testosterone. How many grams of testosterone, C19H28 02 (288.4 g/mol), must be dissolved in 205.0 grams of ethanol to raise the boiling point by 0.350 °C? Refer to the table for the necessary boiling or freezing point constant. Kb (°C/m) Kf(°C/m) Water H₂O 0.512 Ethanol CH3 CH₂OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 Mass= 9 Solvent Formula 1.86 1.99 5.12 M

1. A 0.735 g of a covalent organic compound is dissolved in 15.00 g cyclohexane (freezing point = 6.20 °C). This solution freezes at -7.56°C. The Ki of cyclohexane =20.0°C.kg/mole. What is the molar mass of the solute?

0.263 g of an organic compound (a non-electrolyte) is dissolved in 20.0 g of cyclohexane (C6H12) and the solution freezes at 4.7oC. Pure cyclohexane has a freezing point at 6.5oC and a freezing point depression constant (Kf) of 20.5 oC/m. Calculate the molar mass of the organic compound.            (A) 110 g/mol                            (B) 130 g/mol           (C) 150 g/mol           (D) 210 g/mol

178. Subject  :- Chemistry

A solution is made by dissolving 0.900g of compound Y into 11.000g of cyclohexane. The solution freezes at 3.9 oC. What is the molar mass of compound Y in g/mol?   The Freezing Point of Cyclohexane is 6.6oC. and the freezing point depression constant is kf = 20.0 oC/m. (m=molality). Group of answer choices 0.091 g/mol 606.06 g/mol 303.03 g/mol 1212.12 g/mol

Henry's law may be expressed in different ways and with different concentration units, resulting in different values for the Henry's law constants. If mole fraction is used as the concentration unit, one algebraic statement of the law is: Pgas = KHXgas where k is the Henry's law constant in units of pressure, usually atm. At 25°C, some water is added to a sample of gaseous xenon (Xe) at 3.60 atm pressure in a closed vessel and the vessel is shaken until as much xenon as possible dissolves. Then 2.70 kg of the solution is removed and boiled to expel the xenon, yielding a volume of 1.08 L of Xe (g) at 0 °C and 1.00 atm. Determine the Henry's law constant for xenon in water based on this experiment. atm

Indicate the temperature at which no more than 675 grams of KNO3 can be dissolved in 500 ml of water. (T/I) Solubility (g/L of solvent) 40 °C 70 °C 50 °C 80 °C O 60 °C 1400 1300 1200 1100 1000- 900 800 700 600 500 400 300 200 100 0+ 0 Solubility Curves KI -HCI SO₂ NaNO3 -KNO3 NHẠC KCI -KCIO3 NaCl NH3 10 20 30 40 50 60 70 80 90 100 Temperature (°C)

A solution is prepared by adding 425g of AgNO3 to 0.150L of water at 40.0∘C. The solubility of AgNO3 at 40.0∘C is 311g100.mL. How many grams of AgNO3 are expected to precipitate if the temperature is dropped to 0.00∘C where the solubility of AgNO3 is only 122g100.mL? Give the answer with three significant figures.

What is the freezing point of a solution made by adding 8.93 g bohium flagide to 1 kg of solvent? The freezing point of the solvent is 4.02ºC and the freezing point depression constant of the solvent is 4.11 ºC/m. Report your answer to the hundreths place and do not include units. Use data from the periodic table of Maryland as needed. Element Name Group Number Molar Mass (g/mol) Li Linthium 1 6.276 Na Bohium 1 23.012 K Keysium 1 39.748 Rb Harborium 1 85.729 F Flagine 17 or 7A 18.828 Cl Ceciline 17 or 7A 35.564 Br Baltimine 17 or 7A 78.505 I Chipodine 17 or 7A 122.801