Air is a mixture of gases that is about 78.0% N2 by volume. When air is at standard pressure and 25.0 °C, the N2 component will dissolve in water with asolubility of 4.88 × 10¬4 M. What is the value of Henry's law constant for N2 under these conditions?Express your answer with the appropriate units. Enter the unit M using the compound form mol/L.• View Available Hint(s)k = 6.26 • 10-4MSubmitPrevious AnswersX Incorrect; Try Again; 3 attempts remainingEnter your answer using units of Henry's law constant units.

Given data, There are 78% of N2 present in air by volume. Hence, it means that 78 moles of N2 are…

Answered: Air is a mixture of gases that is about…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 127QRT

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Similar questions

In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure of CO2 in the atmosphere (0.038%, or 0.29 torr), use the Henrys law constant for CO2 in water to estimate the volume of Lake Nyos.
Plants that thrive in salt water must have internal solutions (inside the plant cells) that are isotonic with (have the same osmotic pressure as) the surrounding solution. A leaf of a saltwater plant is able to thrive in an aqueous salt solution (at 25C) that has a freezing point equal to 0.62lC. You would like to use this information to calculate the osmotic pressure of the solution in the cell. a. In order to use the freezing-point depression to calculate osmotic pressure, what assumption must you make (in addition to ideal behavior of the solutions, which we will assume)? b. Under what conditions is the assumption (in part a) reasonable? c. Solve for the osmotic pressure (at 25C) of the solution in the plant cell. d. The plant leaf is placed in an aqueous salt solution (at 25C) that has a boiling point of l02.0C. What will happen to the plant cells in the leaf?
Define the terms in Raoults law. Figure 10-9 illustrates the net transfer of water molecules from pure water to an aqueous solution of a nonvolatile solute. Explain why eventually all of the water from the beaker of pure water will transfer to the aqueous solution. If the experiment illustrated in Fig. 10-9 was performed using a volatile solute, what would happen? How do you calculate the total vapor pressure when both the solute and solvent are volatile?
You dissolve 1.0 mol of urea (H2NCONH2) in 270 g of water. The mole fraction of urea is (a) 3710 3 (b) 0.063 (c) 16 (d) 1.0 and its molality is (a) 1.0 (b) 3.7 (c) 0.063 (d) 0.27
The Henry's law constant for the solubility of radon in water at is 9.57106 M/mm Hg. Radon is present with other gases in a sample taken from an aquifer at 30C. Radon has a mole fraction of 2.7106 in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. (a) molarity (b) ppm (Assume that the water sample has a density of 1.00 g/mL.)
Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.
You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be 0.426C. Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.
(a) If you dissolve 10.0 g (about one heaping teaspoonful) of sugar (sucrose, C12H22O11) in a cup of water (250. g), what are the mole fraction, molality, and weight percent of sugar? (b) Seawater has a sodium ion concentration of 1.08 104 ppm. If the sodium is present in the form of dissolved sodium chloride, what mass of NaCl is in each liter of seawater? Seawater is denser than pure water because of dissolved salts. Its density is 1.05 g/mL

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