Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393600681
Author: Gilbert
Publisher: W. W. Norton & Company
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4. A mixture of helium and neon gases is collected over water at 28.0 °C and 745 mm Hg. If the partial
pressure of helium is 368 mm Hg, what is the partial pressure of neon? (Vapor pressure of water at
28.0 °C = 28.3 mm Hg)
1. Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant?
2. Why does the density of water change with its temperature?
3. If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation?
4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?
13. Consider two containers of volume 1.0 L at 298 K, as shown below. One container holds 0.10 mol N2 and the other holds 0.10 mol H2. The average kinetic energy of the nitrogen molecules is 6.2 X 10 -21 J. Assume that the N2 and the H2 exhibit ideal behavior.
a.
Is the pressure in the container holding the H2 less than, greater than, or equal to the pressure in the container holding the N2. Justify your answer.
b. What is the average kinetic energy of the H2 molecules?
c. The molecules of which gas, N2 or H2, have the greater average speed? Justify your answer.
d. What change could be made that would decrease the average kinetic energy of the molecules in the container?
Chapter 10 Solutions
Chemistry: An Atoms-Focused Approach
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