Question #7 The cooling system in Racer Ralph's car is a mixture of 2.02 kg Compound X and 6.04 kg water. This coolant solution freezes at -16.2 °C. What is the molar mass of Compound X? MM= Data for freezing point K+ (°C/m) boiling point Kb (°C/m) water (H2O) 0.00 °C 1.86 100.00 °C 0.513 g/mol

Question #7 The cooling system in Racer Ralph's car is a mixture of 2.02 kg Compound X and 6.04 kg water. This coolant solution freezes at -16.2 °C. What is the molar mass of Compound X? MM= Data for freezing point K+ (°C/m) boiling point Kb (°C/m) water (H2O) 0.00 °C 1.86 100.00 °C 0.513 g/mol

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 75QAP: A certain gaseous solute dissolves in water, evolving 12.0 kJ of heat. Its solubility at 25C and...

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A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
Caffeine is made up of 49.5% C, 5.2% H, 16.5% O, and 28.9% N. A solution made up of 8.25 g of caffeine and 100.0 mL of benzene (d=0.877g/mL) freezes at 3.03C. Pure benzene (k f =5.10C/m) freezes at 5.500C. What are the simplest and molecular formulas for caffeine?
How many grams of the following nonelectrolytes would have to be mixed with 100.0 g of p-dichlorobenzene to increase the boiling point by 3.0C? To decrease the freezing point by 2.0C? (Use Table 10.2.) (a) succinic acid (C4H6O4) (b) caffeine (C8H10N4O2)
Which of the following salts, Li2SO4 or Cs2SO4, is expected to have the more exothermic enthalpy of hydration?
When KNO3 is dissolved in water, the resulting solution is significantly colder than the water was originally. (a) Is the dissolution of KNO3 an endothermic or an exothermic process? (b) What conclusions can you draw about the intermolecular attractions involved in the process? (c) Is the resulting solution an ideal solution?
Predict the relative solubility of each compound in the two solvents, on the basis of intermolecular attractions. (a) Is NaCl more soluble in water or in carbon tetrachloride? (b) Is I2 more soluble in water or in toluene (C6H5CH3)? (c) Is ethanol (C2H5OH) more soluble in hexane or in water? (d) Is ethylene glycol (HOCH2CH2OH) more soluble in ethanol or in benzene (C6H6)?
Calculate the enthalpies of solution for Li2SO4 and K2SO4. Are the solution processes exothermic or endothermic? Compare them with LiCl and KCl. What similarities or differences do you find?
Two samples of sodium chloride solutions are brought to a boil on a stove. One of the solutions boils at 100.10C and the other at 100.15C. a Which of the solutions is more concentrated? b Which of the solutions would have a lower freezing point? c If you split the solution that boils at 100.1C into two portions, how would the boiling points of the samples compare? Which of the following statements do you agree with regarding the determination of your answer for part c? I. The question cannot be answered with certainty without knowing the volumes of each portion. II. Making the necessary assumption that the two samples have equal volumes, I was able to correctly answer the question. III. The volumes that the sample was split into are irrelevant when determining the correct answer.
Air contains 78% nitrogen. At 25C, Henry's law constant for nitrogen is 6.8104M/atm, while at 37C, it is 6.2104M/atm. (a) How many milligrams of the nitrogen in the air will dissolve in 3.0 L of water at 25C? The air in the head space above the water has a pressure of 1.38 atm. (b) How many milligrams of the nitrogen in the air will dissolve in 3.0 L of water at 37C? The air in the head space above the water has a pressure of 1.38 atm. (c) How much more nitrogen is dissolved at the lower temperature in mass percent?
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
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