What is the freezing point depression (in °C) and freezing point (in K) of a solution containing 2.40 g biphenyl (C₁2H10) in 75.0 g benzene (C6H₁)? Kf (benzene): -5.12 °C kg mol-¹, with a melting temperature of 5.5 °C. a. Freezing point depression: -1.06 °C; freezing point: 277.6 K O b. Freezing point depression: -1.16 °C; freezing point: 277.5 K O C. Freezing point depression: -1.26 °C; freezing point: 277.4 K O d. Freezing point depression: -1.36 °C; freezing point: 277.3 K e. Freezing point depression: -1.46 °C; freezing point: 277.2 K

What is the freezing point depression (in °C) and freezing point (in K) of a solution containing 2.40 g biphenyl (C₁2H10) in 75.0 g benzene (C6H₁)? Kf (benzene): -5.12 °C kg mol-¹, with a melting temperature of 5.5 °C. a. Freezing point depression: -1.06 °C; freezing point: 277.6 K O b. Freezing point depression: -1.16 °C; freezing point: 277.5 K O C. Freezing point depression: -1.26 °C; freezing point: 277.4 K O d. Freezing point depression: -1.36 °C; freezing point: 277.3 K e. Freezing point depression: -1.46 °C; freezing point: 277.2 K

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

the separation of a mixture into pure substance 3. If a solution is made up by mixing 6.0 g of benzoic acid in 1.00 L of water at 42 °C, would the solution be saturated? Would you expect to see solid on the bottom of the container?
Six solutions are made by dissolving a certain amount of each of the six substances in 500. g water. If the freezing point of the each aqueous solution is the same, which substance is added to water in the largest amount, in grams? Assume all ionic compounds dissociate 100% to form ions in solution. ΔT = iKbmsolute ΔT = –iKfmsolute Select one: A. (NH4)2CO3 B. KCl C. The largest mass (g) of substance added is the same for two of the solutions. D.NH4Cl E. Insufficient information is provided. F. NaCl G. CH3OH H. MgCl2 The correct answer should be "B" or KCl, but I don't understand why
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
0.500 g of an unknown nonelectrolyte are dissolved in 25.0 g water. The resulting solution froze at-0.619 °C. Calculate the molar mass of the unknown. Kf (H2O) = 1.86 °C/m O 0.00416 g/mole O 120 g/mole O 0.00832 g/mole O 60.1 g/mole O 30.1 g/mole
Pp
Anthraquinone contains 80.8 % carbon, 3.8 % hydrogen and 15.4 %oxygen. The freezing point of camphor is lowered by 22.3 C when 1.32 g of anthraquinone is dissolved in 11.4 g camphor. (kf = 40.0 C/m, bp = 178.40 C)a. What is the empirical formula of anthraquinone?b. What is the molar mass of anthraquinone?c. What is the molecular formula of anthraquinone?
At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm? solubility: M At 298 K, what is the solubility of oxygen in water exposed to air at 0.893 atm? solubility: M If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from 3.20 L of water in an unsealed container? amount: mol
The boiling point of 500.0L of water was determined to be 100.0°C. Ana has decided to increase the boiling point to 101.0°C by adding ammonium sulfate. How many grams of ammonium sulfate is required to achieve this? (Kb of H20 = 0. 512°C/m; Molar weight of ammeniam sulate=132.14g/mol) A. 119.04 g B. 119.12 g C. 129.04 g D. 129.12 g E. None of the above.
3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small. D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.
Ethylene glycol [CH2(OH)CH2(OH)]is a common automobile antifreeze. The freezing point and boiling point of a solution containing 293 g of ethylene glycol and 1085 g of water are ____and _____ respectively. (Kb and Kf for water are 0.52°C/m and 1.86°C/m, respectively) 8.09 to the power of o space end exponent C comma negative 102.3 to the power of o C negative 9.09 to the power of o space end exponent C comma 112.3 to the power of o C negative 6.09 to the power of o space end exponent C comma 108.3 to the power of o C negative 8.09 to the power of o space end exponent C comma 102.3 to the power of o C
The solubility of ammonium chloride at 70 °C is 60. g of solute per 100 mL of water. Which solution would be exactly saturated at 70 °C? 35 g of solute in 50. mL of water 90. g of solute in 200. mL of water 90. g of solute in 180. mL of water 30. g of solute in 50. mL of water MacBook Air 888 EA F1 F2 F3 F6 F7 F8 F9 F10 F11 @ 2$ 4. 23 % & * 2 3 6 7 8. 9. Q W E Y U
The dissociation of a salt in water to from an aqueous solution is called enthalpy of solution, AHoln- The AH3oln for CaCl, is -120 kJ/mol. When CaCl, is added to water 25. the temperature of the water will increase. the temperature of the water will remain the same. the process is endothermic. nothing will occur, CaCl, is insoluble.