What is the boiling point of a solution that contains 18.7 grams of CCl4 dissolved in 177 grams of ethanol (C2H6O)? For pure ethanol: boiling point = 78.4 °C freezing point = – 114.6  °C Kb  =  1.22 °C/m Kf  =  1.99 °C/m Molar masses: CCl4 = 153.81 g/mol ethanol = 46.08 g/mol Enter your answer to two decimal places.

When 20.0 grams of an unknown compound are dissolved in 500. grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.444°C, and the K₁ for benzene is 5.12°C/m. What is the molar mass of the unknown compound? Hint: Round off to two significant digits. O 110 g/mol Ⓒ 120 g/mol O 130 g/mol O 140 g/mol O None of the above

1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)   2-What is the rate law expression for the reaction A + B → C, based on the following data

A certain liquid X has a normal boiling point of 142.00 °C and a boiling point elevation constant K = 1.03 °C kg-mol A solution is prepared by dissolving some alanine (C₂H,NO₂) in 550. g of X. This solution boils at 143.2 °C. Calculate the mass of C3H-NO, that was dissolved. Round your answer to 2 significant digits. X S

What is the freezing point of a solution containing 0.794 moles of a nonvolatile, non-ionic compound in 271.3 g of liquid benzene? K = 4.90°C/m for benzene, freezing point of benzene is 5.50 °C. Report your answer with the correct number of significant figures. Do not include the unit.

A student dissolves 1.3 g of resveratrol (C₁4H₁203) in 275. mL of a solvent with a density of 1.18 g/mL. The student notices that the volume of the solvent does not change when the resveratrol dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity = molality = 0 x10 0x0 3

A solution of 4.63 g of anhydrous aluminum chloride (AlCl3) in 59.08 g of water freezes at -4.37 degrees celsius. Kf (AlCl3) =1.86 degrees celsius/m part 1: calculate the molar mass of AlCl3 from the formula. Round the answer to the hundredths place. ___ g/mol Part 2: Calculate the molar mass from the freezing point depression, assuming AlCl3 does not dissociate in ions. Round to 3 Significant digits. Part 3: Comparing the two values, how many ions will AlCl3 form? Round the answer to the nearest whole number.

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 425. mL of water at 25.0 °C and a NO partial pressure of 4.98 atm. Round your answer to 2 significant digits. Submit 0 x10 X S

Urea (NH2)2CO, is dissolved in 105.0 g of water. The solution freezes at -0.605°C. How many grams of urea were dissolved to make this solution? The Kf=1.858°C/m for water and its freezing point is 0.000°C. Express your answer to two decimal places.

A solution is made by dissolving 7.80 grams of MgCl2 in 420.0 mL of water. What is the freezing point of this solution (in °C)? Express you answer to 3 significant digits.   Density of water 1.00 g/mL Kf of water 1.86oC/m