Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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4. Calculate the molar concentration of oxygen in water at 25°C for a
partial pressure of 0.22 atm. The Henry's law constant for oxygen is 1.3
x 103 mol/L. atm.
Calculate the mass of oxygen (in mg) dissolved in a 2.50 L bucket of water exposed to a pressure of 2.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Molar mass for oxygen (O2) is 31.9988 g/mol.
A.
46.5 mg
B.
27.0 mg
C.
13.7 mg
D.
23.5 mg
E.
9.87 mg
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.
Chapter 10 Solutions
Chemistry: An Atoms-Focused Approach
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- Use molecular structures and noncovalent interactions to explain why dimethyl ether, (CH3)2O, is completely miscible in water, but dimethylsulfide, (CH3)2S, is only slightly water soluble.arrow_forward4. Calculate the concentration of carbon dioxide in water at 25°C when the pressure of CO2 over the solution is 4.0 atm. The Henry's law constant for CO₂ in water at this temperature is 3.1×10-² mol/L.atm.arrow_forwardExplain the composition and properties of water, the types of bonds between the atoms, characteristics of hydrophilic and hydrophobic molecules.arrow_forward
- Explain the meaning of ‘Equilibrium lattice constant’.arrow_forwardWhich of the following statements regarding solubility of gases in liquids is NOT correct? A. When the Henry’s law constants are given in units of mol/L·atm, larger kH values mean higher solubility. B. The solubility of a gas depends on the identity of the solvent. C. The solubility of gases in water typically decreases as temperature increases. D. The solubility of gases in water typically increases as the mole fraction of the gas above the water’s surface increases. E. The solubility of gases in water typically decreases as the partial pressure of the gas above the water’s surface increasesarrow_forwardAt 25°C Henry's law constant for the solubility of oxygen gas in water is 3.30 x 107 torr. Calculate the solubility of oxygen at room temperature in ppm. Consider air to be 20% O₂ at room temperature. The molar mass of O₂ is 32 g mol-¹.arrow_forward
- X 19. Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 given that kH for O2 is 1.3 × 10-3 M/ atm at this temperature. 23.5 mg a b) 27.3 mg c) 49.4 mg d) 13.7 mg e) 9.87 mgarrow_forwardWhich of the following should have the largest Henry's law constant (kH) in water? CO2 HCl CH4 Ar Xearrow_forwardCalculate 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.arrow_forward
- 3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small. D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.arrow_forwardIn an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the force needed to pull ions apart); the lattice energy, in turn, affects the enthalpy of solution. Based on ion sizes, arrange these compounds by their expected heats of solution. RbCl RbBr Rbl RbF Most exothermic AH soln Most endothermic AH soln Answer Bankarrow_forwardComplete combustion of 8.653 g of a compound of carbon, hydrogen, and oxygen yielded 21.83 g CO₂ and 3.831 g H₂O. When 18.00 g of the compound was dissolved in 288 g of water, the freezing point of the solution was found to be -0.952 °C. For water, Kfp = = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =arrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY