Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393600681
Author: Gilbert
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.
Explain the composition and properties of water, the types of bonds between the atoms, characteristics of hydrophilic and hydrophobic molecules.
Arrange the compounds in order of increasing solubility in water (least soluble first).
HO,
II
HO,
OH
II
IV
O II, I, I, IV
O I, IV, II, III
O IV, I, III, II
O II, I, I, IV
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_forwardDefine the Ground-level ozone, which is the primary component of smog, forms when HC and NOx react in the presence of sunlight on hot, calm days.arrow_forwardCalculate 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 mgarrow_forward
- Mars has a very thin atmosphere with a pressure of 610 Pa, less than 1% of the pressure found on Earth. The atmosphere on Mars is also composed of 95% CO2. Calculate the mass of CO, that would dissolve in 1.0 kg of water on Mars at 0 °C. Data: Henry's Law constant for CO2 at 0 °C is 7.28 x 102 atm 0.44 mg 0.26 mg 19 mg 0.89 mg 7.9 mgarrow_forwardA student investigates the physical and chemical properties of various carbon-containing compounds. Thr complete Lewis electron-dot diagrams and boiling points for two compounds, Q and Z, are shown in the following table: B) Any C — H bond in compound Q is shorter than the S — H bond in compound Z. Explain the reason for this difference using principles of atomic structure.arrow_forwardUse Intermolecular Forces to explain why CF4 is a gas at room temperature but CCl 4 is a liquid.arrow_forward
- Boric acid, B(OH)3 (or H3BO3), does not lose a proton in water, but rather bonds to the O atom of an H2O molecule, which then releases an H+ ion to form the B(OH)4- ion. Use VESPR theory to draw structures, with ideal bond angles, for boric acid and the anion it forms when it reacts with water.arrow_forwardCalculate 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 x 103 M/atm. 49.4 mg 13.7 mg 23.5 mg 9.87 mg O 27.3 mgarrow_forwardThe Henry's law constant for H2 is 8.1×10−4 Matm at 25∘C. What pressure of hydrogen is needed to maintain a H2 concentration of 0.42 M? answer with two significant figures.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