GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
11th Edition
ISBN: 9780134566030
Author: Petrucci
Publisher: PEARSON
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Textbook Question
Chapter 6, Problem 94IAE
Two evacuated bubs of equal volume are connected by a tube of negligible volume. One of the bubs placed in a constant-temperature bath at 225 K and the other bulb is placed in a constant-temperature bath at 350 K. Exactly 1 mol of an ideal gas is injected into the system. Calculate the final number of moles of gas in each bulb.
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A 8.00 L tank at 17.5 °C is filled with 12.8 g of chlorine pentafluoride gas and 4.02 g of carbon dioxide gas. You can
assume both gases behave as ideal gases under these conditions.
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the correct number of significant digits.
olo
mole fraction:
chlorine pentafluoride
partial pressure:
atm
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mole fraction:
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A 1.2 mol sample of oxygen is placed in a 20 L tank at 100 kPa. 1 atm = 101.3 kPa. What is the temperature in the tank?
The ideal gas law, R, can be experimentally determined.
Use the data provided below from the reaction of potassium chlorate decomposing to form oxygen gas and potassium chloride to experimentally determine the value of R in units of L•atm/mol•K.
2KClO3 (s) → 2KCl (s) + 3O2 (g)
The evolved oxygen is collected over water. The relevant data from the experiment is summarized below.
Mass of KClO3 used
0.0665 g
Initial volume reading
46.0 mL
Final volume reading
64.2 mL
Temperature
22.0°C
Total pressure
772.0 mm Hg
A table of vapor pressures of water is also available:
Temperature (°C)
Vapor Pressure of Water (mm Hg)
21
18.7
22
19.8
23
21.1
24
22.4
25
23.8
What is the volume (in L) of O2 gas formed in the experiment?
What is the dry pressure (in mm Hg) of O2 gas in the experiment?
What is the dry pressure (in atm) of O2 gas in the experiment?
What is the temperature (in K) for the experiment?
How many moles of KClO3 were used in this…
Chapter 6 Solutions
GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
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