Calculate the mass of O, that is dissolved in the water inside a 100 L home aquarium at 297 K? Atmospheric pressure is 1.01 bar, the Henry's law constant (kH) for O, at 297 Kis 1.33x10 mol L- bar, the molar mass of O2 is 32.00 g mol', and the atomosphere is 20.95 % O2O 4.28 gO 2.04x10-2gO 0.898 gO 4.28x10-2gO 8.98 g

Given data,Volume of water=100LAtmospheric pressure=1.01barKH=1.33×10-3molL-1bar-1Molar mass of…

Calculate the mass of O, that is dissolved in the water inside a 100 L home aquarium at 297 K? Atmospheric pressure is 1.01 bar, the Henry's law constant (k) for Oz at 297 Kis 1.33x10 mol L- bar. the molar mass of O, is 32.00 g mol, and the atomosphere is 20.05 % O2 O 4.28 g O 2.04x10- a O 0.808 g O 428x10-2g O 8.08 g

Calculate the mass of O, that is dissolved in the water inside a 100 L home aquarium at 297 K? Atmospheric pressure is 1.01 bar, the Henry's law constant (k) for Oz at 297 Kis 1.33x10 mol L- bar. the molar mass of O, is 32.00 g mol, and the atomosphere is 20.05 % O2 O 4.28 g O 2.04x10- a O 0.808 g O 428x10-2g O 8.08 g

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 89QAP

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In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560 g of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 L water per day. a. Assuming all of the dissolved solids are MgCO3 and assuming a temperature of 27C, what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60 M NaCl.)
Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL
Argon makes up 0.93% by volume of air. Calculate its solu-bility (mol/L) in water at 20°C and 1.0 atm. The Henry’s lawconstant for Ar under these conditions is 1.5X10⁻³ mol/Latm.
1.) Are there any intermolecular forces (IMF’s) between water molecules and cyclohexane molecules? What kind(s)? Given this, what would the magnitude and sign of DHMIXING be for cyclohexane dissolving in water? a) Are there any IMF’s between water molecules and other water molecules? What kind(s)? Given this, what would the magnitude and sign of DHSOLVENT be for cyclohexane dissolving in water? c) Are there any IMF’s between cyclohexane molecules and other cyclohexane molecules? What kind(s)? Given this, what would the magnitude and sign of DHSOLUTE be for cyclohexane dissolving in water? d) Why do you think cyclohexane does not dissolve in water? Analyze this the way it was done in class, thinking about the three contributions to DHSOLUTION. What do you think the magnitude and sign of DHSOLUTION would be for dissolving cyclohexane in water? (Explain.) Would you expect these substances to dissolve in each other? Why?
CO2 in water has a Henry’s law constant KB = 1.25 × 106 torr. How many liters of CO2 are needed to make 1 liter of sparkling water at 1 atm and 300 K? The density of water is 1 kg/L and it does not change as CO2 is dissolved. N.B. Treat gas as a solute, and note that in order for water to “sparkle” the partial pressure of CO2 in the vapor phase must equal the atmospheric pressure (note that this neglects the partial pressure of the water vapor).
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A sample of carbon dioxide occupies a volume of 3.5 liters at 125 kPa pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters? With solution
A piece of metal "X" weighing 0.0382 g was placed in an eudiometer containing dilute aqueous HCI. After the metal fully dissolved ,15.4 mL of hydrogen gas was collected by displacement of water and a 400 mm column of water was observed. The water temperature was 25 degrees Celcius and the barometric pressure was 758.8 mm Hg ( torr). Refer to the introduction and data sheet to solve the following problems. a) Calculate the volume occupied by the hydrogen gas at STP. b) How many moles of the metal were consumed in the reaction? c) What is the molar mass of the metal?
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(a) If a 500-mL glass beaker is filled to the brim with ethyl alcohol at a temperature of 5.00oC how much will overflow when its temperature reaches 22.0oC? (b) How much less water would overflow under the same conditions?
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Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have mole fraction of methane = 0.915 and mole fraction of ethane = 0.085. (a) What are the partial pressure of the two gases in a 14.10 L container of natural gas at 30 degrees Celcius and 1.34 atm? (b) Assuming complete combustion of both gases in the natural gas sample, what is the total mass of water formed? Hint: Write the balanced combustion chemical equation for each gas separately in the gas mixture to find the mass of water formed.

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