Calculating partial pressure in a gas mixture GHA 0/5 A 8.00 L tank at 24.9 °C is filled with 9.56 g of boron trifluoride gas and 4.99 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. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm

Q: A 10.0 L tank at 22.7 °C is filled with 4.77 g of sulfur tetrafluoride gas and 11.0 g of dinitrogen…

A: Mole fraction is the ratio of umber of moles of a constituent to the sum of all the number of moles…

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: www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-lg O STATES OF MATTER Calculating mole fraction in a gas…

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Q: please help me. double and triple check your answers, previous tutors got it wrong.

A: The mole fraction of C2H4O2 is calculated as,

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…

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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 6.00 L tank at 0.87 °C is filled with 10.1 g of boron trifluoride gas and 8.92 g of sulfur…

A: Given  Data  6.0 Litre 0.87 °C 10.1 gram of BF3 and 8.92 gram SF6 Calculation  of partial  pressure…

Q: Many water treatment plants use chlorine gas to kill mi-cro organisms before the water is released…

A: From ideal gas law, PV = nRT , P = (80 / 100 ) × 85  = 68 atm,  T = 298 K , R = 0.082 L , V = 850 L…

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 5.00 L tank at 8.29 °C is filled with 9.60 g of sulfur hexafluoride gas and 9.76 g of chlorine…

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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: 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: 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 10.0 L tank at 7.69 °C is filled with 10.8 g of sulfur tetrafluoride gas and 2.28 g of dinitrogen…

A: We have to calculate the mole fraction, partial pressure and total pressure.

Q: A 7.00 L tank at 20. °C is filled with 14.6 g of sulfur tetrafluoride gas and 5.63 g of sulfur…

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Q: Calculate the mole faction and partial pressure of each gas and the total pressure in the tank round…

A: First, the moles of carbon monoxide gas and carbon dioxide gas are determined by using given mass…

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 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 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: 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…

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Q: A 10.0 L tank at 4.23 "C is filled with 7.60 g of chlorine pentafil gases under these conditions.…

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Q: A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 g of chlorine…

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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 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 mixture of methane (CH4) and ethane (C2H6) is stored in a container at 294 mm Hg. The gases are…

A: The reactions taking place will be  CH4 + 2 O2 ----> CO2 + 2 H2O And 2 C2H6 + 7 O2 -------> 4…

Q: Rank the following gases from least dense to most dense at 1.00 atm and 298 K: SO2, HBr, CO2.…

A: Given,SO2,HBr,CO2At 1.00 atm and 298 K

Q: • Assuming that a 1.5g gas occupying a volume of 500ml at a pressure of 175 atm and a temperature of…

A: Mass of gas = 1.5 g  Volume of gas (V) = 500 mL = 0.5 L  Pressure of gas ( P)= 175 atm  Temperature…

Q: A 7.00 L tank at 21.9 °C is filled with 5.47 g of sulfur hexafluoride gas and 5.98 g of boron…

A: Given : Volume of tank = 7.00 L Temperature = 21.9 oC Mass of sulfur hexafluoride i.e SF6 = 5.47 g…

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…

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Q: Calculate the mole fraction and partial pressure of each gas and the total pressure in the tank.

A: First, the moles of dinitrogen difluoride gas and sulfur hexafluoride gas are determined by using…

Q: A 9.00 L tank at 4.22 °C is filled with 3.83 g of sulfur tetrafluoride gas and 7.58 g of sulfur…

A: In this case, we first we will find total pressure, then partial pressure of each species using mole…

Q: Carbon dioxide lasers are used as cutting tools and industry medicine and his research instruments…

A: From Dalton's law we can calculate the pressure of the different components .

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: 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: O STATES OF MATTER Calculating mole fraction in a gas mixture A 8.00 L tank at -3.4 °C is filled…

A: Given :-  Mass of BF3 = 9.03 g  Mass of N2O = 4.25 g  Volume of tank = 8.00 L  Temperature = -3.4°C…

Q: A 10.0 L tank at 0.6 °C is filled with 3.23 g of sulfur tetrafluoride gas and 17.3 g of dinitrogen…

A: Given: Volume of tank = 10.0 L Temperature = 0.6 oC Mass of sulfur hexafluoride i.e. SF6 = 3.23 g.…

Q: A 6.00 L tank at 0.46 °C is filled with 7.03 g of dinitrogen difluoride gas and 3.38 g of sulfur…

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Q: A 10.0 L tank at 8. °C is filled with 17.7 g of sulfur hexafluoride gas and 5.37 g of boron…

A: Given: Volume of tank = 10.0 L Temperature = 8 oC Mass of sulfur hexafluoride i.e. SF6 = 17.7 g. And…

Q: A 10.0 L tank at 26.1 °C is filled with 12.8 g of dinitrogen difluoride gas and 3.26 g of dinitrogen…

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Q: Find the volume (in m3) of 28 mole Nitrogen GAS maintained at 15 degree celcius at an absolute…

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Q: A 10.0 L tank at 6.06 °C is filled with 18.1 g of chlorine pentafluoride gas and 5.47 g of boron…

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Q: A 5.00L tank at 0.7°C is filled with 16.5g of dinitrogen difluoride gas and 5.00g of sulfur…

A: Calculation for moles of dinitrogen difluoride:

Q: is filled with  6.16g  of sulfur hexafluoride gas and  18.8g  of dinitrogen difluoride gas. You…

A: To solve this problem first we will calculate the mole fraction using the number of moles of each…

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

A: Dalton's law: Dalton's law of partial pressures states that in a mixture of non-reacting gases, the…

Q: A 6.00 L tank at 17.7 °C is filled with 4.59 g of dinitrogen monoxide gas and 10.3 g of sulfur…

A: Given data :  1. Volume = 6.00L  2.Temperature =17.7 oC =(17.7+273)K…

Q: At a certain temperature, 20g of CO2 gas(MM = 44.01g/mol) at 2.15atm take up a volume of 5.25mL.…

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Q: A 5.00L tank at 0.1°C is filled with 19.4g of dinitrogen monoxide gas and 5.47g of boron trifluoride…

A: Please find the solution below:

Q: A 8.00L tank at 24.1°C is filled with 8.62g of boron trifluoride gas and 7.37g of sulfur…

A: The mass of boron trifluoride gas is = 8.62 g The mass of sulfur tetrafluoride gas is = 7.37 g We…

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

A: So we will determine the mole fraction and partial pressure for Nitrogen and oxygen gas.

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.