Open Question
Why do fish die when placed in a tank filled with water that has been boiled and then cooled?
Ch.13 - Solutions
Chapter 13, Problem 49
Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium, assuming a total pressure of 1.0 atm and a mole fraction for nitrogen of 0.78.
Verified step by step guidance1
Identify the relevant law: Use 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.
Calculate the partial pressure of nitrogen: Multiply the total pressure by the mole fraction of nitrogen, i.e., \( P_{\text{N}_2} = 1.0 \text{ atm} \times 0.78 \).
Use Henry's Law to find the concentration of nitrogen: \( C = k_H \times P_{\text{N}_2} \), where \( k_H \) is the Henry's Law constant for nitrogen at room temperature.
Determine the volume of water in the aquarium: Since the aquarium is 80.0 L, assume this is the volume of water available for dissolving nitrogen.
Calculate the mass of nitrogen: Use the concentration from Henry's Law and the volume of water to find the moles of nitrogen, then convert moles to mass using the molar mass of nitrogen (28.02 g/mol).
Related Practice
Open Question
Scuba divers breathing air at increased pressure can suffer from nitrogen narcosis—a condition resembling drunkenness—when the partial pressure of nitrogen exceeds about 4 atm. What property of gas-water solutions causes this to happen? How can a diver reverse this effect?
Textbook Question
Scuba divers breathing air at increased pressure can suffer from oxygen toxicity—too much oxygen in their bloodstream— when the partial pressure of oxygen exceeds about 1.4 atm. What happens to the amount of oxygen in a diver's bloodstream when he or she breathes oxygen at elevated pressures? How can this be reversed?
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Textbook Question
An aqueous NaCl solution is made using 112 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molarity of the solution. (Assume a density of 1.08 g/mL for the solution.)
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Textbook Question
An aqueous NaCl solution is made using 112 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molality of the solution. (Assume a density of 1.08 g/mL for the solution.)
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Textbook Question
An aqueous NaCl solution is made using 112 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the mass percent of the solution. (Assume a density of 1.08 g/mL for the solution.)
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