Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 1, Problem 1.12E
Interpretation Introduction
Interpretation:
The value of constant in equation 1.9 for a 1.887 mol gas sample with a pressure of 2.66 bar, a volume of 27.5 L and a temperature of 466.9 K is to be calculated. The answer is to be compared with the values in Table 1.2.
Concept introduction:
The
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 113. kPa.
The piston is now pulled up, expanding the gas, until the gas has a final volume of 20.0 L. Calculate the final pressure of the gas. Be sure your answer haş the
correct number of significant digits.
piston
cylinder
gas
olo
Ar
||kPa
x10
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
=
O Gases
Calculating partial pressure in a gas mixture
tab
sulfur tetrafluoride
E.H
chlorine pentafluoride
Explanation
A 8.00 L tank at 29.8 °C is filled with 14.2 g of sulfur tetrafluoride gas and 13.7 g of chlorine pentafluoride 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. Round each of your answers to 3 significant digits.
Esc
Check
1
Type here to search
Total pressure in tank:
F1
mole fraction:
partial pressure:
Q
mole fraction:
partial pressure:
@
2
F2
W
F3
#
3
E
J
0
0
atm
0
0a
9x
atm
atm
F4
$
4
R
FS
TI
X
F
%
012
5
50%
T
F6
3
A
6
G
F7
Y
&
7
H
FB
*
8
athenaCollector v2.
4
4
J
FO
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
57°F Cloudy ^ 40
10:31 AM
11/13/2023
O
(
prt sc
9
F10
5
home
athenaCollector v2...
O
K
F11
OI
1/5
end
F12
P
D
3
Danasia V
All Booken
insert
=
?
alo
Ar
back
Chapter 1 Solutions
Physical Chemistry
Ch. 1 - A bomb calorimeter is a study metal vessel in...Ch. 1 - Difference between the system and the...Ch. 1 - Prob. 1.3ECh. 1 - Prob. 1.4ECh. 1 - Prob. 1.5ECh. 1 - Prob. 1.6ECh. 1 - Prob. 1.7ECh. 1 - A pot of cold water is heated on a stove, and when...Ch. 1 - hat difference is necessary for heat to flow...Ch. 1 - What is the value of FT for a sample of gas whose...
Ch. 1 - What is the value of FP for a sample of gas whose...Ch. 1 - Prob. 1.12ECh. 1 - Hydrogen gas is used in weather balloon because it...Ch. 1 - Prob. 1.14ECh. 1 - A 2.0 L soda bottle is pressurized with 4.5 atm of...Ch. 1 - The Mount Pinatubo volcano eruption in 1991...Ch. 1 - Prob. 1.17ECh. 1 - Scottish physicist W. J. M. Rankine proposed an...Ch. 1 - Use the two appropriate values of R to determine a...Ch. 1 - Prob. 1.20ECh. 1 - Pressures of gases in mixtures are referred to as...Ch. 1 - Earths atmosphere is approximately 80 N2 and 20...Ch. 1 - The atmospheric surface pressure on Venus is 90...Ch. 1 - Prob. 1.24ECh. 1 - Prob. 1.25ECh. 1 - In the anaerobic oxidation of glucose by yeast,...Ch. 1 - What are the slopes of the following lines at the...Ch. 1 - For the following function, evaluate the...Ch. 1 - Determine the expressions for the following,...Ch. 1 - Determine the expressions for the following,...Ch. 1 - Prob. 1.31ECh. 1 - Prob. 1.32ECh. 1 - Prob. 1.33ECh. 1 - Prob. 1.34ECh. 1 - What properties of a nonideal gas do the Vander...Ch. 1 - Prob. 1.36ECh. 1 - Prob. 1.37ECh. 1 - Calculate the Boyle temperatures for carbon...Ch. 1 - Prob. 1.39ECh. 1 - Prob. 1.40ECh. 1 - Table 1.4 show that the second virial coefficient...Ch. 1 - Prob. 1.42ECh. 1 - What is the van der Waals constant a for Ne in...Ch. 1 - Prob. 1.44ECh. 1 - Under what conditions would the van der Waals...Ch. 1 - By definition, the compressibility of an ideal gas...Ch. 1 - The second virial coefficient B and the third...Ch. 1 - Use the approximation 1 x-1 1 x x2 to...Ch. 1 - Why is nitrogen a good choice for the study of...Ch. 1 - Evaluate for a gas following the Redlich-Kwong...Ch. 1 - Numerically evaluate for one mole of methane...Ch. 1 - Under what conditions of volume does a van der...Ch. 1 - At high temperatures, one of the van der Waals...Ch. 1 - Under what conditions of temperature does a...Ch. 1 - The Berthelot equation of state for one mole of...Ch. 1 - Prob. 1.56ECh. 1 - Referring to exercises 1.6 and 1.7, does it matter...Ch. 1 - Prob. 1.58ECh. 1 - Use Figure 1.11 to construct the cyclic rule...Ch. 1 - Prob. 1.60ECh. 1 - Prob. 1.61ECh. 1 - Calculate for one mole of an ideal gas at STP and...Ch. 1 - Prob. 1.63ECh. 1 - Show that = T/p for an ideal gas.Ch. 1 - Determine an expression for V/T p, n in terms of ...Ch. 1 - Prob. 1.66ECh. 1 - Prob. 1.67ECh. 1 - Perform a units analysis on the exponent of the...Ch. 1 - Using the barometric formula, calculate the...Ch. 1 - The barometric formula can also be used for...Ch. 1 - Prob. 1.71ECh. 1 - Prob. 1.72ECh. 1 - Prob. 1.73ECh. 1 - Prob. 1.74ECh. 1 - Prob. 1.75ECh. 1 - Prob. 1.76ECh. 1 - Prob. 1.77ECh. 1 - Prob. 1.78ECh. 1 - Prob. 1.79ECh. 1 - Use the ideal gas law to symbolically prove the...Ch. 1 - Prob. 1.81E
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A 9.00 L tank at 1.5 °C is filled with 3.22 g of carbon monoxide gas and 16.7 g of chlorine pentafluoride 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. carbon monoxide chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm x10 × Ś 0:39 0 Earrow_forwardA 7.00 L tank at 25.9 °C is filled with 7.99 g of sulfur hexafluoride gas and 4.45 g of dinitrogen monoxide 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. sulfur hexafluoride dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atmarrow_forwardA 7.00 L tank at 19. °C is filled with 7.37 g of sulfur hexafluoride gas and 6.63 g of sulfur tetrafluoride 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. sulfur hexafluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: a atm 0 atm atm x10 X Śarrow_forward
- Calculate the partial pressure of each component in a mixture of gases contains 3.50 g N2, 2.50 g H2, and 5.27 g of NH3, if the temperature is 25 Celcius and the volume of the mixture is 1.00 L. Please help me solve this one with steps. I thought that it would be the same as calculating with moles, but I'm not even sure anymore.arrow_forwardA 10.0 L tank at 19.1 °C is filled with 6.04 g of dinitrogen difluoride gas and 7.73 g of chlorine pentafluoride 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. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: | atmarrow_forward8.) A 1.08 mol sample of Ar gas is confined in a 25.9 liter container at 19.1 °C.If 1.08 mol of Ne gas is added holding the volume and temperature constant, the average kinetic energy of the total system will a. not enough information to answer the question b. remain the same c. increase d. decreasearrow_forward
- Experiments carried out by French chemists Jacques Alexandre César Charles and Joseph-Louis Gay-Lussac and British physicist Lord Kelvin determined a quantitative relationship between the volume and temperature of a gas. Their data showed that for a container of gas held at constant pressure, the volume and temperature are directly proportional. For example, if you inflate a balloon outdoors with cold air on a cold day and then take it inside, it will expand, and it might even burst. This happens because as the temperature of the air inside the balloon increases, the volume of the balloon increases as well. What is less obvious is the quantitative relation: If the pressure is held constant, then when the temperature is doubled, the volume is doubled as well. Part A According to Charles's law, for a fixed quantity of gas at constant pressure, which of the given quantities is constant? ► View Available Hint(s) OF O VXT O V +T Submit Part B A balloon was filled to a volume of 2.50 L when…arrow_forwardA 10.0 L tank at 2.5 °C is filled with 17.5 g of chlorine pentafluoride gas and 3.17 g of boron trifluoride 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. mole fraction: x10 chlorine pentafluoride partial pressure: ? atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm Oarrow_forwardThis relationship is known as Graham’s Law of Effusion. Since both gases are at the same temperature, they must have the same average kinetic energy (½ mv2), where m is mass and v is velocity (like speed). Since both gases have the same average kinetic energy, you can state that ½ mLvL2 = ½ mHvH2. Multiplying both sides by 2 gives you mLvL2 = mHvH2. Rearranging the equation to get both masses on the same side of the equation will give you mL/mH = VH2/VL2. In 3a and 3b, you probably noticed that the heavy gas particles took twice as long to diffuse as the light gas particles. This means that the light gas particles are moving twice as fast, VH/VL = ½. Therefore, VH2/VL2 = ¼. If the light gas was Ne, what would be a reasonable identity for the heavy gas? Explain.arrow_forward
- A 7.00 L tank at 18.3 °C is filled with 17.0 g of sulfur tetrafluoride gas and 15.2 g of chlorine pentafluoride 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. sulfur tetrafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 atm atm atm x10 Xarrow_forwardA 10.0 L tank at 6.69 °C is filled with 7.02 g of carbon dioxide gas and 4.65 g of sulfur hexafluoride 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. mole fraction: carbon dioxide partial pressure: |atm mole fraction: sulfur hexafluoride partial pressure: |atm Total pressure in tank: atmarrow_forwardA 5.00 L tank at 8.18 °C is filled with 17.3 g of sulfur tetrafluoride gas and 4.95 g of chlorine pentafluoride 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. sulfur tetrafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 atm atm atm x10 X Śarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning