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 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 dinitrogen difluoridel sulfur hexafluoride mole fraction X S 2 do Ar

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 26.2 °C is filled with 3.15 g of dinitrogen monoxide gas and 17.6 g of boron…

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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 7.00 L tank at 3.16 °C is filled with 2.08 g of boron trifluoride gas and 6.38 g of sulfur…

A: We have given that  Volume of tank = 7.0 L  Temperature = 3.16 °C = 276.16 K  Mass of BF3 = 2.08 g…

Q: Calculating partial pressure in a gas mixture Jacqueline v A 10.0 L tank at 7.37 °C is filled with…

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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: 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 20.1 °C is filled with 10.5 g of sulfur hexafluoride gas and 6.52 g of dinitrogen…

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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 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 10.00 L tank at 11.0 °C is filled with 4.26 g of dinitrogen difluoride gas and 5.33 g of carbon…

A:

Q: A 5.00 L tank at 28. °C is filled with 16.8 g of chlorine pentafluoride gas and 5.27 g of sulfur…

A: Information of question

Q: 9.00L tank at −10.7°C is filled with 7.23g of chlorine pentafluoride gas and 7.49g of sulfur…

A: A numerical problem based on gas law, which is to be accomplished.

Q: A5.00 L tank at 12.0 °C is filled with 2.83 g of sulfur tetrafluoride gas and 13.3 g of carbon…

A:

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…

A:

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 10.00 L tank at 21.4 °C is filled with 14.8 g of carbon monoxide gas and 10.7 g of sulfur…

A:

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

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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…

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Q: A 6.00L tank at 24.1°C is filled with 12.2g of dinitrogen monoxide gas and18.1g of carbon dioxide…

A: The mass of dinitrogen is = 12.2 g The mass of carbon dioxide is = 18.1 g dinitrogen mole fraction…

Q: A 6.00 L tank at 22.1 °C is filled with 12.0 g of sulfur tetrafluoride gas and 2.42 g of carbon…

A: Given information: Mass of sulfur tetrafluoride = 12.0 g Mass of carbon dioxide = 2.42 g

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…

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

A:

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: 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: mole fraction

A:

Q: A 7.00 L tank at 18.8 °C is filled with 6.41 g of boron trifluoride gas and 17.6 g of chlorine…

A: Given information is as follows: The volume of the tank = 7.00 L The temperature of the tank = 18.8…

Q: A 7.00 L tank at -10.6 °C is filled with 12.1 g of sulfur hexafluoride gas and 10.0 g of dinitrogen…

A:

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 7.00 L tank at 29.4 °C is filled with 2.63 g of sulfur hexafluoride gas and 12.9 g of boron…

A: Volume of tank (V) = 7.0 L                 Temperature (T) = 29.4oC…

Q: A 9.00 L tank at 8.36 °C is filled with 4.08 g of sulfur hexafluoride gas and 10.8 g of boron…

A:

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: Calculating partial pressure in a gas mixture A 8.00 L tank at 9.28 °C is filled with 6.17 g of…

A: The objective of this question is to calculate the mole fraction, partial pressure of each gas, and…

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: 10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 g of sulfur…

A: Given: Volume of tank = 10.0 L Mass of dinitrogen difluoride = 15.4 g Mass of sulfur tetrafluoride…

Q: A  7.00L  tank at  0.68°C  is filled with  7.59g  of boron trifluoride gas and  17.5g  of…

A:

Q: A 7.00 L tank at 5.2 °C is filled with 11.2 g of chlorine pentafluoride gas and 15.0 g of dinitrogen…

A:

Q: A 5.00 L tank at 15.3°C is filled with 6.86 g of dinitrogen monoxide gas, 12.5 g of sulfur…

A: Formula used   X( mole fraction) = mole ÷total moles moles = mass÷molar mass

Q: A 9.00 L tank at 14.3 °C is filled with 3.65 g of sulfur tetrafluoride gas and 3.18 g of carbon…

A: The volume of the tank = The mass of the sulfur tetrafluoride gas = The mass of the carbon dioxide…

Q: A 10.0L tank at 9.41°C is filled with 4.32g of carbon dioxide gas and 4.99g of sulfur hexafluoride…

A: Given: Volume of tank = 10.00 L Temperature of gas = 9.41 oC Mass of CO2 i.e. carbon dioxide gas =…

Q: A 6.00 L tank at 16.8 °C is filled with 2.62 g of carbon dioxide gas and 5.02 g of sulfur…

A: Mass of Carbon dioxide (CO2) = 2.62 gMass of sulfur tetrafluoride (SF4) = 5.02 gMole fraction of…

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.