General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
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.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have
the correct number of significant digits.
olo
mole fraction:
chlorine pentafluoride
partial pressure:
atm
Ar
mole fraction:
carbon dioxide
partial pressure:
atm
Total pressure in tank:
atm
For ideal gases with each of the following sets of P, V, n, and T, determine the missing number. Note that these different sets of numbers are not related to one another. Pay attention to the units.
PS: Make sure that you have rearranged the equation properly. If you start from the PV=nRT form of the equation, you should never have to do anything other than dividing to isolate the variable of interest. Also, make sure you are using the proper value of R. To do so, make sure the units line up with the data that is given in the question.
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
How many moles of KClO3 were used in this experiment?
many moles of O2 gas were evolved in this experiment?
What is the experimentally determined value of the ideal gas law constant, R, expressed in L•atm/mol•K?
Chapter 6 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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The "initial"...Ch. 6 - Two evacuated bubs of equal volume are connected...Ch. 6 - Prob. 95IAECh. 6 - A 0.7178 g sample of a hydrocarbon occupies a...Ch. 6 - Prob. 97IAECh. 6 - Ammonium nitrite, NH4NO2,decomposes according to...Ch. 6 - A mature of 100 g H2 and 860 g O2, introduced into...Ch. 6 - Prob. 100IAECh. 6 - What is the partial pressure of CI2(g) , in...Ch. 6 - Prob. 102IAECh. 6 - When working with a mixture of gases, it is...Ch. 6 - Prob. 104IAECh. 6 - Gas cylinder A has e volume of 48.2 L and contains...Ch. 6 - Prob. 106IAECh. 6 - Producer gas is a type of fuel gas made by passing...Ch. 6 - Prob. 108IAECh. 6 - A mixture of H2(g) and O2(g) is prepared by...Ch. 6 - Prob. 110IAECh. 6 - Prob. 111IAECh. 6 - A breathing mixture is prepared which He is...Ch. 6 - Chlorine dioxide,CIO2, is sometimes used as a...Ch. 6 - The amount of ozone, O2,in a mixture of gases can...Ch. 6 - Prob. 115IAECh. 6 - Prob. 116IAECh. 6 - We have noted that atmospheric pressure depends on...Ch. 6 - Consider a sample ofO2(g) at 298 K and 1.0 atm....Ch. 6 - A nitrogen molecule (N2) having the average...Ch. 6 - Prob. 120IAECh. 6 - Prob. 121IAECh. 6 - Prob. 122IAECh. 6 - Prob. 123IAECh. 6 - A 0.156 g sample of magnesium-aluminum alloy...Ch. 6 - Prob. 125FPCh. 6 - Prob. 126FPCh. 6 - Prob. 127FPCh. 6 - Prob. 128FPCh. 6 - Prob. 129FPCh. 6 - Prob. 130SAECh. 6 - Briefly describe each concept or process: (a)...Ch. 6 - Prob. 132SAECh. 6 - Which exerts the greatest pressure. 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