Skip to main content
Pearson+ LogoPearson+ Logo
Ch.13 - Solutions & Their Properties
All textbooksMcMurry 8th EditionCh.13 - Solutions & Their PropertiesProblem 86
Chapter 13, Problem 86

Sulfur hexafluoride, which is used as a nonflammable insulator in high-voltage transformers, has a Henry’s law constant of 2.4 * 10⁻⁴ mol/L·atm at 25 °C. What is the solubility in mol/L of sulfur hexafluoride in water at 25 °C and a partial pressure of 2.00 atm?

Verified step by step guidance
1
Identify the given values: Henry's law constant \( k_H = 2.4 \times 10^{-4} \text{ mol/L·atm} \) and the partial pressure \( P = 2.00 \text{ atm} \).
Recall Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The formula is \( S = k_H \times P \), where \( S \) is the solubility.
Substitute the given values into the Henry's Law equation: \( S = (2.4 \times 10^{-4} \text{ mol/L·atm}) \times (2.00 \text{ atm}) \).
Perform the multiplication to find the solubility \( S \) in mol/L.
Interpret the result to understand the solubility of sulfur hexafluoride in water under the given conditions.
Related Practice
Open Question
Hydrogen sulfide, H₂S, is a toxic gas responsible for the odor of rotten eggs. The solubility of H₂S in water at STP is 0.195 M. What is the Henry’s law constant of H₂S at 0 °C? What is the solubility of H₂S in water at 0 °C and a partial pressure of 25.5 mm Hg?
Textbook Question
Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxygen above the water in atmospheres at 0 °C is needed to obtain this concentration? The solubility of O2 in water at 0 °C and 1 atm partial pressure is 2.21 * 10-3 mol>L.
843
views
Textbook Question
At an altitude of 10,000 ft, the partial pressure of oxygen in the lungs is about 68 mm Hg. What is the concentration in mg/L of dissolved O2 in blood (or water) at this partial pres- sure and a normal body temperature of 37 °C? The solubil- ity of O2 in water at 37 °C and 1 atm partial pressure is 1.93 * 10-3 mol>L.
888
views
Textbook Question
When 1 mL of toluene is added to 100 mL of benzene (bp 80.1 °C), the boiling point of the benzene solution rises, but when 1 mL of benzene is added to 100 mL of toluene (bp 110.6 °C), the boiling point of the toluene solution falls. Explain.
836
views
Open Question
When solid CaCl2 is added to liquid water, the temperature rises. When solid CaCl2 is added to ice at 0 °C, the temperature falls. Explain.
Open Question
Which of the following aqueous solutions has the (a) higher freezing point, (b) higher boiling point, (c) lower vapor pressure: 0.50 m sucrose (C12H22O11) or 0.35 m HNO3?