CHEMISTRY 161 CHAPTER #10 in class problems MARCH 18, 2014 1. Arterial blood contains about 0.25 g of Oxygen per liter at 37°C and standard atmospheric pressure. a. What is the Henry’s law constant (mole/L-atm) for oxygen dissolved in blood? The mole fraction for oxygen in air is 0.209. b. Use Henry’s law constant for oxygen dissolved in arterial blood to calculate the solubility of oxygen in the blood of a climber on top of Mount Everest if the atmospheric pressure is 0.35 atm. c. Use Henry’s law constant for oxygen dissolved in arterial blood to calculate the solubility of oxygen in the blood of a scuba diver 90 feet below the ocean surface if the pressure is 3 atm (pressure of water and scuba tank air) 2. Circle the salt of the highest melting point from the pairs listed below. a. NaCl and KCl b. NaCl and NaBr c. CaCl2 and CaSO4 d. Al2(SO4)3 or CaSO4 3. Which sulfur oxide would you predict to be more soluble in nonpolar solvents: SO 2 or SO3? 4. Using the phase diagram below answer the following question. a. At room temperature is carbon dioxide a solid, liquid, or a gas? b. Estimate the boiling and freezing points of carbon dioxide. c. Will solid carbon dioxide float or sink in liquid carbon dioxide? 5. Explain why van der Waals constant a for CO2 is smaller than SO2?