A 10.0 L tank at 28.9 °C is filled with 7.97 g of sulfur tetrafluoride gas and 15.3 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. Round each of your answers to 3 significant digits. mole fraction: sulfur tetrafluoride partial pressure: atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

PV = nRT Number of mol = Mass/molar mass Mole fraction of ith species (Xi) = ni/n , where n = total…

Answered: A 10.0 L tank at 28.9 °C is filled with 7.97 g of sulfur tetrafluoride gas and 15.3 g of sulfur hexafluoride gas. You can assume both gases behave as ideal…

Chemistry

10th Edition

ISBN: 9781305957404

Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher: Cengage Learning

See similar textbooks

Related questions

Q: A 7.00 L tank at 6.29 °C is filled with 14.0 g of sulfur hexafluoride gas and 2.97 g of dinitrogen…

Q: A 10.0 L tank at 4.55 °C is filled with 6.12 g of boron trifluoride gas and 12.3 g of sulfur…

Q: A 6.00 L tank at 0.95 °C is filled with 2.17 g of dinitrogen monoxide gas and 7.50 g of sulfur…

Q: A 10.0 L tank at 12.5 °C is filled with 3.91 g of sulfur tetrafluoride gas and 6.79 g of dinitrogen…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 3.91 g Mass of dinitrogen monoxide i.e N2O = 6.79 g…

Q: A 6.00 L tank at 12.2 °C is filled with 5.23 g of chlorine pentafluoride gas and 13.7 g of boron…

A: Ideal gas equation: PV = nRT P = Pressure V = Volume n = Total number of moles R = Gas constant T…

Q: Calculating partial pressure in a gas mixture 0/5 A 8.00 L tank at 24.9 °C is filled with 9.56 g of…

Q: A 6.00 L tank at 11. °C is filled with 12.3 g of sulfur hexafluoride gas and 5.56 g of chlorine…

A: A 6.00 L tank at 11. °C is filled with 12.3 g of sulfur hexafluoride gas and 5.56 g of chlorine…

Q: A9.00 L tank at 15.1 °C is filled with 19.7 g of boron trifluoride gas and 4.20 g of dinitrogen…

A: The volume of the tank = Temperature = Mass of The molar mass of Mass of Molar mass of

Q: A 7.00 L tank at 7.57 °C is filled with 4.38 g of dinitrogen monoxide gas and 2.99 g of boron…

Q: A 7.00 L tank at 20.1 °C is filled with 10.5 g of sulfur hexafluoride gas and 6.52 g of dinitrogen…

Q: A 6.00 L tank at 10.1 °C is filled with 7.51 g of boron trifluoride gas and 2.21 g of carbon dioxide…

A: It is based on the concept of mole fraction and Dalton's law of partial pressure Here we are…

Q: 8.00 L tank at 0.72 °C is filled with 10.9 g of boron trifluoride gas and 7.07 g of dinitrogen…

A: Given : Mass of BF3 = 10.9 g Mass of dinitrogen monoxide = 7.07g

Q: A 9.00 L tank at 22.7 °C is filled with 6.21 g of sulfur hexafluoride gas and 7.82 g of boron…

Q: A 5.00 L tank at 12. °C is filled with 14.2 g of chlorine pentafluoride gas and 3.58 g of sulfur…

Q: A 6.00 L tank at 8.97 °C is filled with 5.16 g of sulfur tetrafluoride gas and 6.76 g of boron…

Q: A 10.0 L tank at 23.7 °C is filled with 5.14 g of boron trifluoride gas and 13.4 g of dinitrogen…

Q: ome N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: Total pressure (P) = 0.060 Kpa

Q: A 5.00 L tank at 4.58 °C is filled with 15.2 g of chlorine pentafluoride gas and 7.62 g of sulfur…

A: Ideal gas equation: PV = nRT P = Pressure V = Volume n = Number of moles R = Gas constant T =…

Q: A 8.00 L tank at 7.11 °C is filled with 8.60 g of boron trifluoride gas and 5.95 g of carbon dioxide…

A: Given that: Volume of the tank, V = 8.00 LTemperature, T = 7.11oC = (273.15 + 7.11) K = 280.26 KMass…

Q: A 6.00 L tank at 18.4 °C is filled with 6.85 g of boron trifluoride gas and 18.4 g of carbon dioxide…

A: A 6.00 L tank at 18.4 °C is filled with 6.85 g of boron trifluoride gas and 18.4 g of carbon dioxide…

Q: A 8.00 L tank at 0.07 °C is filled with 4.49 g of chlorine pentafluoride gas and 16.3 g of sulfur…

A: Molar mass of ClF5 is 130.445 g/mol and molar mass of SF4 is 108.07 g/mol. Given temperature is…

Q: A 6.00 L tank at 0.29°C is filled with 5.04g of chlorine pentafluoride gas and 11.9g of sulfur…

A: Number of moles of a substance is equal to the mass of the substance divided by its molar mass.…

Q: A 9.00 L tank at 12. °C is filled with 17.4 g of dinitrogen difluoride gas and 9.28 g of sulfur…

Q: A 6.00 L tank at 24.2 °C is filled with 5.19 g of sulfur hexafluoride gas and 19.5 g of chlorine…

A: Given that : The volume of the tank = 6.00 L Temperature = 24.2°C The mass of sulfur hexafluoride =…

Q: A 9.00 L tank at 28.9 °C is filled with 8.24 g of sulfur tetrafluoride gas and 5.83 g of chlorine…

A: Volume of the tank = 9 LTemperature = 28.9 0CAmount of sulfur tetrafluoride = 8.24 gAmount of…

Q: A 10.0 L tank at 2.58 °C is filled with 14.4 g of sulfur hexafluoride gas and 2.83 g of dinitrogen…

A: Given, volume of the tank =10.0 Ltemperature T =2.58 °C =(2.58+273.15) K =275.73 Kamount of sulfur…

Q: A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 g of dinitrogen…

Q: A 10.00 L tank at -2.9 °C is filled with 11.6 g of boron trifluoride gas and 3.29 g of dinitrogen…

Q: A 6.00 L tank at 29.9 °C is filled with 6.33 g of sulfur tetrafluoride gas and 12.3 g of sulfur…

Q: A 10.0 L tank at 1.79 °C is filled with 8.09 g of chlorine pentafluoride gas and 14.0 g of…

Q: A 8.00 L tank at -8.3 °C is filled with 15.2 g of dinitrogen monoxide gas and 8.30 g of boron…

A: The first step is to calculate the number of moles of each gas. The number of moles can be…

Q: A 9.00L tank at 8.48°C is filled with 10.9g of sulfur hexafluoride gas and 8.24g of sulfur…

Q: A 5.00 L tank at 1.0 °C is filled with 6.54 g of sulfur hexafluoride gas and 15.5 g of boron…

Q: A 10.00 L tank at 8.3 °C is filled with 4.02 g of chlorine pentafluoride gas and 4.69 g of…

Q: A 9.00 L tank at 1.9 °C is filled with 15.6 g of dinitrogen difluoride gas and 11.7 g of sulfur…

Q: A 8.00 L tank at 4.12 °C is filled with 11.7 g of chlorine pentafluoride gas and 14.1 g of boron…

A: The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a…

Q: A 7.00 L tank at 0.15 °C is filled with 11.0 g of sulfur hexafluoride gas and 3.66 g of carbon…

Q: A 6.00L tank at 18.5°C is filled with 2.08g of boron trifluoride gas and 18.9g of sulfur…

A: Volume of tank (V) = 6.0 L Temperature (T) = 18.5oC…

Q: A 8.00 L tank at 4.28 °C is filled with 8.76 g of dinitrogen monoxide gas and 9.81 g of boron…

Q: A 6.00 L tank at 18.3 °C is filled with 4.33 g of carbon dioxide gas and 7.47 g of sulfur…

Q: Some Ny gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: In a mixture of various gas, mole fraction can be calculated as the ratio of moles of a particular…

Concept explainers

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases…

Question

100%

A 10.0 L tank at 28.9 °C is filled with 7.97 g of sulfur tetrafluoride gas and 15.3 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. Round each of your answers to 3 significant digits.
mole fraction:
x10
sulfur tetrafluoride
partial pressure:
atm
mole fraction:
sulfur hexafluoride
partial pressure:
atm
Total pressure in tank:
atm

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution

See solution Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW