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 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: dinitrogen monoxide atm partial pressure: atm Total pressure in tank:

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

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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…

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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 9.00 L tank at 4.88 °C is filled with 12.4 g of boron trifluoride gas and 7.92 g of sulfur…

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Q: A 5.00 L tank at 4.81 °C is filled with 17.5 g of sulfur hexafluoride gas and 4.15 g of chlorine…

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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…

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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…

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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…

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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…

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Q: A7.00 L tank at 9.77 "C is filled with 7.38 g of sulfur hexafluoride gas and 14.8 g of dinitrogen…

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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…

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Q: A 9.00 L tank at 5.13 °C is filled with 9.94 g of dinitrogen monoxide gas and 16.9 g of sulfur…

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Q: A 10.0 L tank at 17. °C is filled with 9.03 g of dinitrogen monoxide gas and 6.93 g of chlorine…

A: Given that -  Volume of the tank = 10.0 L  Temperature = 17.0°C = 273+17 = 290 K  Weight of…

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

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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…

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Q: A 9.00 L tank at 23.9 °C is filled with 6.76 g of boron trifluoride gas and 4.61 g of sulfur…

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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…

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Q: A 8.00 L tank at 6.68 °C is filled with 11.4 g of dinitrogen difluoride gas and 6.23 g of chlorine…

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

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Q: A 9.00 L tank at 5.07 °C is filled with 4.41 g of sulfur hexafluoride gas and 11.0 g of carbon…

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Q: A 10.0 L tank at 5.62 °C is filled with 4.36 g of carbon monoxide gas and 6.20 g of sulfur…

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

A: To calculate the partial pressure of each gas present in the container, one uses Dalton's Law of…

Q: A 8.00 L tank at 8.19 °C is filled with 11.2 g of sulfur tetrafluoride gas and 13.1 g of boron…

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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…

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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: A 6.00 L tank at 26.7 °C is filled with 2.28 g of sulfur hexafluoride gas and 2.26 g of chlorine…

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Q: A 6.00 L tank at 26.7 °C is filled with 2.28 g of sulfur hexafluoride gas and 2.26 g of chlorine…

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Q: Mariales at 4.58 °C is filled with 15.2 g of sulfur hexafluoride gas and 5.64 g of boron trifluoride…

A: Applying formulas: PA = nART/V ;  PB= nBRT/V  PT = PA + PB  PA = XA. Ptotal   ; PB= XB. Ptotal

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: 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…

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Q: A 5.00 L tank at 7.12 °C is filled with 8.00 g of sulfur hexafluoride gas and 5.34 g of dinitrogen…

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Q: A 5.00 L tank at 5.3 °C is filled with 14.5 g of sulfur tetrafluoride gas and 4.33 g of chlorine…

A: A 5.00 L tank at 5.3 oC is filled with 14.5 g of sulfur tetrafluoride gas and 4.33 g of chlorine…

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 10.0 L tank at 3.85 °C is filled with 10.3 g of sulfur hexafluoride gas and 6.25 g of dinitrogen…

A: Number of moles of sulfur hexafluoride can be calculated as, Number of moles of SF6=MassMolar…

Q: A 7.00 L tank at 29, °C is filled with 6.44 g of chlorine pentafluoride gas and 13.6 g of boron…

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Q: A 5.00 L tank at 14.6 °C is filled with 2.51 g of dinitrogen monoxide gas and 10.8 g of chlorine…

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Q: A8.00 L tank at 8.88 °C is filled with 3.30 g of carbon dioxide gas and 13.9 g of dinitrogen…

A: Given- Volume=8.00L  Weight of carbon dioxide= 3.30g Weight of dinitrogen difluoride gas= 13.9g…

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

A: The total pressure of the mixture = 1100. torrCalculation of the mole fraction and partial pressure…

Q: A 9.00 L tank at 2.97 °C is filled with 18.5 g of sulfur tetrafluoride gas and 9.86 g of sulfur…

A: We can express mole fraction in terms of moles of individuals and total moles of gas molecules…

Q: A 9.00 L tank at 9.39 °C is filled with 6.14 g of dinitrogen monoxide gas and 9.14 g of boron…

A: Number of moles of N2O = mass/mol.wt. = 6.14 g/(44.01 g/mol) = 0.139514 mol  Number of moles of BF3…

Q: A 6.00 L tank at 4.54 °C is filled with 5.68 g of boron trifluoride gas and 19.3 g of sulfur…

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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. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.