MISSED THIS? Watch KCV Colligative Properties Read Section 14.6. You can click on the Review link to access the section in your e Text An aqueous solution containing 35.0 g of an unknown molecular (non-electrolyte) compound in 151.8 g of water was found to have a freezing point of -1.3°C Calculate the molar mass of the unknown compound (Use Kf = 1.86 °C/m) Express your answer using two significant figures. G| ΑΣΦ M Submit = 3.9 Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining ? g/mol

MISSED THIS? Watch KCV Colligative Properties Read Section 14.6. You can click on the Review link to access the section in your e Text An aqueous solution containing 35.0 g of an unknown molecular (non-electrolyte) compound in 151.8 g of water was found to have a freezing point of -1.3°C Calculate the molar mass of the unknown compound (Use Kf = 1.86 °C/m) Express your answer using two significant figures. G| ΑΣΦ M Submit = 3.9 Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining ? g/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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If the freezing point of the solution was observed to be -8.6 °C, and the normal freezing point of cyclohexane is 6.50 °C, what is the value of Kf for cyclohexane? 4.67 g of toluene in 67.8 g of cyclohexane The molar mass of toluene is 92.14 g/mol.
✓mall amount of acetonitrile (CH₂CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) CH₂CN 98 B H₂O Use these sketches to answer the questions in the table below. The enthalpy of solution AH soln is negative when CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. Would heat be absorbed or released if the system moved from Stage A to B? What force would oppose or favor the system moving from Stage A to B? Check all that apply. 0 O absorbed O released O neither absorbed nor released none Olonic bonding force O covalent bonding force metal bonding force Ohydrogen-bonding force dipole force ion-dipole force Odispersion force 0.0. X solution. S
Submit Question 17 of 20 In reverse osmosis, water flows out of a salt solution until the osmotic pressure of the solution equals the applied pressure. Assume seawater has a colligative molarity of 1.10 M, and you want to use reverse osmosis to produce freshwater from the seawater. Calculate the volume of seawater (in liters) required to produce 10.0 liters of freshwater when a pressure of 65 atm is applied to the seawater at 25°C. The ideal gas constant is 0.08205 L·atm/mol K. 1 3 C 8 +/- x 100 2. 4- 7.
1 4 7 8 When 2.19 g of a certain molecular compound X are dissolved in 100. g of formamide (NH, COH), the freezing point of the solution is measured to be - 0.4 °C. Calculate the molar mass of X. If you need any additional information on formamide, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits. Submit Assign Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acces
Calculate the freezing point of a solution that contains 168.4 g of sucrose (table sugar) in 300. g of water. One mole of sucrose is 342 g. Kf for H2O = 1.86°C/m -0.185 oC -3.05 oC -0.558 oC -0.744 oC -1.24 oC
A 3.40-g sample of a mixture of naphthalene (C10H8) and pyrene (C16H10) is dissolved in 35.0 g benzene (C6H6). The freezing point of the solution is 2.23°C. What is the mass (in grams) of the naphthalene in the sample mixture? The freezing point of benzene is 5.51°C and Kf is 5.12°C kg/mol.
Menthol is a crystalline substance with a peppermint taste and odor. When 1.18 g of menthol is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 6.31 °C. Look up the freezing point and Kf constant for cyclohexane in the Colligative Constants table. Calculate the molar mass of menthol. molar mass: g/mol Question Source: MRG- General Chemistry Publisher: University Scie labout us .careers: privacy policy terms of use contact us help MacBook
When 0.258 g of a molecular compound, benzoic acid, was dissolved in 40.0 g of benzene, the freezing point of the solution was lowered to 5.23 °C. What is the molecular weight of the benzoic acid? Kf= 5.12°C/m, freezing point benzene = 5.51°C
23. An ethylene glycol solution contains 28.3 g of ethylene glycol, C2H602 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.
A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 43.33 g L.. The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 3.1 g.1.¹. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Round each of your answers to 2 significant digits. 0% 0.8 X 5
b. When 4.35 grams of ethylene glycol (C2HO2) is dissolved in 100g of water, the resulting solution gas a freezing point of -1.31°C. Calculate the molar mass of ethylene glycol.
1. Suppose that you add 27.5 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 3.58 oC compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound? 2. What is the freezing point (in degrees Celcius) of 3.70 kg of water if it contains 187.4 g of CaBr2? The freezing point depression constant for water is 1.86 oC/m and the molar mass of CaBr2 is 199.89 g/mol. 3. What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -5.6 °C? The freezing point depression constant of water is 1.86 ºC/m.