One of the detrimental effects of the "thermal pollution" of water supplies is that a rise in temperature reduces the amount of dissolved oxygen available to fish. Using the information in the table of Henry's Law constants (K) below, calculate how many litres of water a fish requires at 30.0°C to obtain the same amount of oxygen that it could obtain from 3.05 L of water at 25.0°C. TABLE HENRY'S LAW CONSTANTS (KH) IN AQUEOUS SOLUTION (M/Bar) Gas 0.0 °C 25 °C 30 °C N2 1.1 x 10-3 6.6 x 10-4 4.0 x 10-4 O2 2.5 x 103 1.3 x 10-3 8.8 x 10-4 CO 1.6 x 103 9.5 x 104 4.4 x 10-4 Ar 2.5 x 10-3 1.5 x 10-3 1.0 x 10-3 Не 4.1 x 10-4 3.8 x 10-4 3.8 x 10-4 CO2 7.7 × 10-2 3.4 x 10-2 1.6 x 10-2 i 1.7

One of the detrimental effects of the "thermal pollution" of water supplies is that a rise in temperature reduces the amount of dissolved oxygen available to fish. Using the information in the table of Henry's Law constants (K) below, calculate how many litres of water a fish requires at 30.0°C to obtain the same amount of oxygen that it could obtain from 3.05 L of water at 25.0°C. TABLE HENRY'S LAW CONSTANTS (KH) IN AQUEOUS SOLUTION (M/Bar) Gas 0.0 °C 25 °C 30 °C N2 1.1 x 10-3 6.6 x 10-4 4.0 x 10-4 O2 2.5 x 103 1.3 x 10-3 8.8 x 10-4 CO 1.6 x 103 9.5 x 104 4.4 x 10-4 Ar 2.5 x 10-3 1.5 x 10-3 1.0 x 10-3 Не 4.1 x 10-4 3.8 x 10-4 3.8 x 10-4 CO2 7.7 × 10-2 3.4 x 10-2 1.6 x 10-2 i 1.7

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 freezing point of water H₂O is 0.00 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in water is antifreeze (ethylene glycol). How many grams of antifreeze, CH₂ OHCH₂OH (62.10 g/mol), must be dissolved in 268.0 grams of water to reduce the freezing point by 0.450 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb(°C/m) Kf(°C/m) Water H₂O 0.512 Ethanol CH3 CH₂ OH 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 Mass= g 1.86 1.99 5.12
The vapor pressure of water is 23.76 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in water is glucose.Calculate the vapor pressure of the solution at 25 °C when 6.800 grams of glucose, C6H12O6 (180.2 g/mol), are dissolved in 267.7 grams of water.water = H2O = 18.02 g/mol.VP(solution) = mm Hg
The partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 4.3 atm. What is the solubility of CO2 in champagne? Assume the Henry's law constant is the same for champagne as it is for water: at 20°C, kH = 3.7 × 10−2 mol/(L·atm).
The Henry's law constant for O₂ in water at 25°C is 1.28 x 10³ M/atm, and the mole fraction of O₂ in the atmosphere is 0.21. Calculate the solubility of O₂ in water at 25°C at an atmospheric pressure of 1.00 atm
Calculate the solubility of O2 in water at a partial pressure of O₂ of 150. torr at 25°C. The Henry's law constant for O₂ is 1.3 x 10-3 mol/L atm for Henry's law in the form C = KP, where C js the gas concentration (mol/L). Solubility= mol/L
The freezing point of benzene CGH6 is 5.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in benzene is DDT. How many grams of DDT, C14H,Cl5 (354.5 g/mol), must be dissolved in 207.0 grams of benzene to reduce the freezing point by 0.400°C ? Refer to the table for the necessary boiling or freezing point constant. Formula | K, (°C/m) Kf(°C/m) Solvent Water H20 0.512 1.86 Ethanol CH;CH,OH 1.22 1.99 Chloroform CHC13 3.67 Benzene CH6 2.53 5.12 Diethyl ether CH;CH,OCH,CH3 2.02 g DDT.
As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.69 atm and a temperature of 25.0 °C, what is the solubility of N2 in a diver's blood? [Use the value of the Henry's law constant k calculated in Part A, 6.26 x 10-4 mol/(L· atm).JAssume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood. Express your answer with the appropriate units.
The solubility of Ne in water at 25 °C is 2.1 × 10⁻⁴ M when the partial pressure of Ne is 0.20 atm. What is the value of the Henry's law constant for Ne?
Calculate the dissolved oxygen in mg/L at an altitude of 1,000 m above sea level that has an atmospheric pressure of 0.89 atm; assuming constant temperature of 25 °C. The Henry Law constant (kH) for the solubility of O2 in water at 25 ° C is 1.3 x 10-3 mol/L.atm.
6. An alkene is reacted with Br2 to yield two stereospecific products. The same alkene is reacted with HCl and yields four stereospecific products. Draw the alkene. Upload Choose a File
Calculate the solubility of oxygen in water at the top of Mt. Everest where the atmospheric pressure is 0.370 atm. The mole fraction of O2 in air is 0.209. Assume the kH of O2 is 1.30 ×× 10–3 mol/(L • atm).
Calculate the osmotic pressure of a solution containing 18.45 mg of hemoglobin in 15.7 mL of solution at 35 ∘C. The molar mass of hemoglobin is 6.5×104 g/mol. Express your answer in atmospheres.