Macmillan Learning A 6.41 L cylinder contains 1.55 mol of gas A and 3.63 mol of gas B, at a temperature of 27.0 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior. PA = PB = What is the total pressure? PTotal = kPa kPa kPa

Macmillan Learning A 6.41 L cylinder contains 1.55 mol of gas A and 3.63 mol of gas B, at a temperature of 27.0 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior. PA = PB = What is the total pressure? PTotal = kPa kPa kPa

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: If a gaseous mixture is made by combining 2.15 g Ar and 3.13 g Kr in an evacuated 2.50 L container…

Q: A certain gas sample has a volume of 225 mL at a pressure of 1.25 atm at 27oC; what would be its…

A: Given: P1 = 1.25 atm V1 = 225 ml P2 = 0.75 atm V2 = ? according to boyles at constant temperature.…

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: At 8°C a 1.0-L flask contains 1.0 x 10-2 mole of N2, 4.0 x 102 mg O2, and 4.7 x 1021 molecules of…

Q: A gas mixture in a 3.900 L container at 305°C contains 1.20 g each of Ar, CO, and CH4. Find the…

A: We have given that Volume of gas mixture = 3.9 L Temperature of Gas mixture = 3050C = 578 K Mass of…

Q: A 5.00 L tank at 23.6 °C is filled with 3.92 g of dinitrogen monoxide gas and 19.6 g of sulfur…

A: Given, Mass of dinitrogen monoxide (N2O) gas = 3.92 g Mass of sulfur hexafluoride (SF6) gas = 19.6…

Q: A gas sample originally occupies 436 mL at 24 °C. When the volume is expanded to 612 mL and the…

A: The ideal gas equation is given by,

Q: A 5.00 L tank at 8.05 °C is filled with 5.82 g of sulfur tetrafluoride gas and 10.1 g of boron…

A: Volume (V) = 5.00 L tank at Temperature (T) = 8.05 °C sulfur tetrafluoride = 5.82 gboron…

Q: Part 1. A chemist reacted 12.0 liters of F2 gas with NaCl in the laboratory to form Cl2 gas and NaF.…

A: Given: Volume (V), F2 used = 12 L The pressure (P) = 1.5 atm Temperature (T) = 28 K Standard P, T…

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 gas sample is collected in a 0.249 L container at 28.1 °C and 0.912 bar. If the sample has a mass…

A: Using law of Ideal gas, we can determine the moles of gas present in the sample. Ideal gas law- PV…

Q: A 10.0 L tank at 1.79 °C is filled with 15.7 g of sulfur tetrafluoride gas and 15.1 g of dinitrogen…

A: Moles of SF4 = 15.7 g /108gmol-1 = 0.145 mol Moles of N2F2 = 15.1 g /66…

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

A: The mole fractions are calculated using the following formulae. Mole fraction of N2=Number of N2…

Q: Sulfur tetrafluoride gas is collected at −4.0°C in an evacuated flask with a measured volume of…

A: Applying ideal gas equation PV = nRT where P= pressure, V= volume, n= no. of moles R= gas…

Q: A 8.00 L tank at 6.9 °C is filled with 9.35 g of carbon dioxide gas and 9.40 g of dinitrogen…

A: Mole fraction of different gases can be calculated by knowing the total moles of gases and the moles…

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 5.00 L tank at 29.6 °C is filled with 17.3 g of boron trifluoride gas and 12.8 g of chlorine…

Q: Suppose that Daniel has a 2.50 L bottle that contains a mixture of O₂, N₂, and CO₂ under a total…

A: Since you have posted multiple questions, we can solve only the first question for you according to…

Q: A 10.00 L tank at 29.5 °C is filled with 5.59 g of sulfur tetrafluoride gas and 12.5 g of carbon…

A: mass of Carbon dioxide (CO2) = 12.5 gmass of sulfur tetrafluoride (SF4) = 5.59 gMole fraction of…

Q: A 6.00 L tank at 6.88 °C is filled with 4.07 g of sulfur tetrafluoride gas and 5.51 g of boron…

A: given mass of SF4 = 4.07 g mass of BF3 = 5.51 g temperature = 6.88°C volume = 6 L

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…

Q: A 7.00 L tank at 12.3 °C is filled with 12.8 g of sulfur hexafluoride gas and 15.5 g of sulfur…

A: Given: Volume of tank = 7 L Temperature = 12.3°C=12.3+273.15 K=285.45 K Mass of sulfur hexafluoride…

Q: Calculating mole fraction in a gas mixture A 9.00 L tank at 26.9 °C is filled with 11.0 g of sulfur…

A: Mass of boron trifluoride = 4.84g Mass of sulfur hexafluoride = 11.0 g Molar Mass of boron…

Q: A 10.0 L tank at 6.25 °C is filled with 8.59 g of carbon dioxide gas and 3.67 g of chlorine…

A: Gases present : CO2 (carbon dioxide) and ClF5 (chlorine pentafluoride) Temperature = 6.25 oC Volume…

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

A: Information about the question

Q: A 6.00 L tank at 18.3 °C is filled with 4.25 g of sulfur tetrafluoride gas and 7.37 g of boron…

Q: A 10.0 L tank at 24.7 °C is filled with 11.0 g of dinitrogen difluoride gas and 13.1 g of sulfur…

A: The combined relation between gas laws is known as the ideal gas law or the gas equation. The…

Q: A 9.00 L tank at 24.6 °C is filled with 7.29 g of dinitrogen monoxide gas and 5.10 g of dinitrogen…

Q: 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…

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

Q: A 7.13 L cylinder contains 1.82 mol of gas A and 3.77 mol of gas B, at a temperature of 31.8 °C.…

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: container was filled with 0.893 moles of N2, 0.687 moles of O2, 0.734 moles of H2, and 0.248 moles…

Q: A 8.00 L tank at 18. °C is filled with 6.96 g of dinitrogen difluoride gas and 11.8 g of chlorine…

A: The total pressure present in the tank can be calculated using the ideal gas law equation which is…

Q: A gas mixture in a 1.65-L container at 294 K contains 10.0 gg of Ne and 10.0 g of Ar. Calculate the…

Q: Some N, gas is mixed with some 0, gas, and the sketch below shows a representative sample of the…

A: Number of O2 molecules = 14 Number of N2 molecules = 6 Total number of molecules = 14 +6 = 20 Mole…

Q: If a gaseous mixture is made by combining 1.29 g Ar and 2.46 g Kr in an evacuated 2.50 L container…

A: The total pressure of a mixture of two non reacting gases is given by PtotalV = (n1+n2)RT Ptotal =…

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

A: The mole fractions are calculated using the following formulae.

Q: A gas mixture in a 3.700 L container at 460°C contains 1.20 g each of Ar, CO, and CH4. Find the…

A: Total volume of gas mixture = 3.7 L Temperature = 460◦C or 733.15 K Gas constant, R = 0.0821…

Q: A 9.00 L tank at 27. °C is filled with 5.07 g of dinitrogen difluoride gas and 3.97 g of sulfur…

A: Ideal gas equation: PV = nRT P = pressure, V = volume , n = moles, R = gas constantT =…

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

A: The number of N2 gas molecules is 14.The number of O2 gas molecules is 6.The total pressure is 2.50…

Q: A 6.00 L tank at 9.98 °C is filled with 8.79 g of sulfur hexafluoride gas and 5.44 g of carbon…

A: Below attached file showing the details answer All the best .

Q: A sample of a smokestack emission was collected into a 1.10-L tank at 742 mm Hg and analyzed. The…

A: In 100 g sample mass of CO2= 92 g Mass of NO = 4.2 g Mass of SO2 =1.3g Mass of H2O = 2.5g Molar…

Q: A 7.00 L tank at 25.3 °C is filled with 6.94 g of carbon dioxide gas and 3.83 g of chlorine…

Q: A 10.00 L tank at 15.8 °C is filled with 9.68 g of sulfur hexafluoride gas and 13.2 g of boron…

Q: Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right).…

A: The values are provided in questionReaction takes place at atmosphere pressure P = 1 atm Temperature…

Q: A 9.00 L tank at 22.4 °C is filled with 11.2 g of boron trifluoride gas and 13.3 g of sulfur…

A: Volume of tank = 9L Temperature = 22.4°C or 295.55K Mass of boron trifluoride = 11.2g Mass of…

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

Question

Macmillan Learning
A 6.41 L cylinder contains 1.55 mol of gas and 3.63 mol of gas B, at a temperature of 27.0 °C. Calculate the partial pressure
of each gas in the cylinder. Assume ideal gas behavior.
PA =
PB =
What is the total pressure?
PTotal =
kPa
kPa
kPa

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

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

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 6.00 L tank at 14.3 °C is filled with 18.2 g of carbon monoxide gas and 17.0 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction ? carbon monoxide sulfur tetrafluoride
A 10.0 L tank at 2.46 °C is filled with 18.0 g of boron trifluoride gas and 7.03 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. mole fraction: x10 boron trifluoride 18 Ar partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm
A 10.0 L tank at 8.65 °C is filled with 6.29 g of boron trifluoride gas and 8.89 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 in the tank. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: sulfur hexafluoride partial pressure: atm 24 Mac DD 80 F10 11 F7 F8 F9 F4 F5 F2 F3
An unknown gas at 79.1 °C and 1.05 atm has a molar mass of 44.10 g/mol. Assuming ideal behavior, what is the density of the gas? density: g/L Enter numeric value
Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 3.00 atm. key carbon hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure x10 N₂ 02 atm ☐ ☑ atm
A 10.0 L tank at 18.9 °C is filled with 13.1 g of sulfur hexafluoride gas and 6.12 g of carbon 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. Round each of your answers to 3 significant digits. mole fraction: sulfur hexafluoride partial pressure: atm mole fraction: carbon monoxide partial pressure: I atm atm Total pressure in tank:
A 6.00 L tank at -2.4 °C is filled with 2.01 g of sulfur tetrafluoride gas and 6.11 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas sulfur tetrafluoride sulfur hexafluoride mole fraction 0 0 X Ś 0 000 13 Ar
A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 g of dinitrogen difluoride 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. ol. mole fraction: x10 chlorine pentafluoride Ar ? partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm
A 9.00 L tank at 3.79 °C is filled with 8.94 g of sulfur tetrafluoride gas and 13.3 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. sulfur tetrafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atm X
A 9.00 L tank at 6.02 °C is filled with 8.81 g of sulfur hexafluoride gas and 10.5 g of dinitrogen difluoride 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 hexafluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm
A 5.00 L tank at 29.4 °C is filled with 19.9 g of sulfur tetrafluoride gas and 4.02 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction sulfur tetrafluoride chlorine pentafluoride
Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 0.150 kPa. gas N₂ 0₂ carbon nitrogen kPa oxygen mole fraction partial pressure kPa key Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. hydrogen x10 sulfur chlorine × Ś