A. Critical point: 374 C, 218 atm. B. Liquid is more dense variation. C. Triple point: - 56.4 C, 5.11 atm. D. Freezing point depression. 7. Describe the INCORRECT colligative properties observed when non-volati solute is added to the solvent. A. Catalytic converter. B. Boiling point elevation. C. Vapour pressure lowering. D. Freezing point depression. 8. Select the CORRECT definition of eutectic mixture. A. Liquid that has higher boiling point and remains as liquid after the distillation. B. A mixture of two or more phases at a composition that has the lowest melti point. CFree eneray change for the formation of 1 mole of the substance from

A. Critical point: 374 C, 218 atm. B. Liquid is more dense variation. C. Triple point: - 56.4 C, 5.11 atm. D. Freezing point depression. 7. Describe the INCORRECT colligative properties observed when non-volati solute is added to the solvent. A. Catalytic converter. B. Boiling point elevation. C. Vapour pressure lowering. D. Freezing point depression. 8. Select the CORRECT definition of eutectic mixture. A. Liquid that has higher boiling point and remains as liquid after the distillation. B. A mixture of two or more phases at a composition that has the lowest melti point. CFree eneray change for the formation of 1 mole of the substance from

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...

See similar textbooks

Similar questions

Which of the following statements is considered true? a. For common liquids, the normal freezing points and normal boiling points are constant b. the molal boiling point elevation and freezing point depression constants for a given solvent carry the unit of measurement of degrees C/molarity c. A and B are correct d. A and B are incorrect
Match the following aqueous solutions with the appropriate letter from the column on the right. 1.8.75x10-2 m AICI 3 A. Highest boiling point KNO3 K₂S B. Second highest boiling point C. Third highest boiling point D. Lowest boiling point Ethylene glycol (nonelectrolyte) 2.0.160 m 3.0.127 m 4.0.410 m
The deviation of the van’t Hoff factor from ideal values indicates: a. Non-equilibrium conditions b. Low temperature conditions c. High pressure conditions d. A protic solvent e. Incomplete dissociation of solute
The change in vapor pressure (AP) between that of the solution and pure solvent is directly proportional to the - O a. vapor pressure of the solute O b. vapor pressure of the solution O c. mole fraction of solute in the solution O d. mole fraction of solvent in the solution
Choose the colligative property that utilize the ideal gas equation in its calculation. Select one: O a. Vapour pressure lowering O b. Boiling point elevation O c. Freezing depression O d. Osmotic pressure
What is boiling point? What is freezing point? What is dissolution? Effects and relevance of the dissolution of a solid in water to different industries in our day-to-day lives. How is freezing point/boiling point related?
40. 5.63 grams of LiBr is dissolved in 78.0 grams of water. What is the mole fraction of LiBr in this solutic a. 0.00955 b. 0.0122 c. 0.0147 d. 0.0173 41. "The tendency of atoms in molecules to have eight electrons in their valence shells" is the b. valence a. eight c. full shell d. octet 42. A solution consists of sodium chloride solid dissolved in water. How will the solubility of the sodium affected by the increase in pressure above the solution? a. It will increase. b. It will decrease. c. It will remain unchanged. 回 t M Address X S
9. If 528 mg of an unknown sample was dissolved in 10.00 of t-butanol (CAH9OH) and the freezing point decreased by 3.46°C the apparent molar mass from this data is A. 133 grams/mole. B. 139 grams/mole. C. 143 grams/mole D. 147 grams/mole. E. 157 grams/mole. grams
All of the colligative properties can be explained thermodynamically as solute particles.. a) Increasing the S of the liquid phase b)Increasing the H of the liquid phase c) Decreasing the H of the liquid phase d)Decreasing the S of the liquid phase
1. Fill in the blanks in the table for aqueous solutions of the compounds shown. The density of the solution is in g/mL. Abbreviations: m is molality, Mass % is the mass percentage of the solute, Mole Frac. is the mole fraction of the solute, and M is molarity of the solute. Compound f.w. d. soln. 62.07 17.03 56.11 HỌC H,CH,OH NH3 KOH 1.0460 0.9228 1.3444 m 14.68 Mass % 36.00 Mole Frac. M 8.626
Non-volatile solutes are the required solutes for the colligative property on boiling point because these solutes lower the vapor pressure of the solution. Thus, A. also lowers the boiling point of the solutionB. a higher temp causes the solution to boilC. both solute and solvent will not remain in solutionD. lowering the vapor pressure of the solvent
D. Freezing Point Calculation Directions: Study the sample problem and do the task given. Sample problem with solution, Task to do Ethylene glycol (C2H6O2) is a molecular compound Calculate the freezing point of a solution that is used in many commercial anti-freezes. An aqueous solution of ethylene glycol is used in. vehicle radiators to prevent the water in the radiator from freezing by lowering its freezing point. Calculate the freezing point of a solution of 400. g of ethylene glycol in 500.g of water. repared by dissolving 27.56 g of glucose (C6H1206) into 125 g of water. Step 1: List the known quantities and plan the problem. Step 1: Kf (H2O) = -1.86 °C/m %3D Known: mass of C2H6O2 = 400. g molar mass of C2H6O2 = 62.08 g/mol mass of H20 = 500. g = 0.500 kg Kf (H20) = -1.86 °C/m *Kf- is the constant freezing point %3D %3D %3D %3DD ni noiulge Unknown: Tf of solution = ? °C *Tf- is the total freezing point This is a three-step problem. First, calculate the moles of ethylene glycol.…