Some Ny 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 0.060 kPa. gas N₂ 0₂ carbon nitrogen oxygen key mole fraction partial pressure 0 0 kPa kPa O Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 2 significant digits. You may assume each gas behaves as an ideal gas. hydrogen sulfur chlorine X

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…

A:

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

A:

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

A: The total number of gas molecules are 20.  Total number of oxygen molecules = 17 Total number of…

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…

A:

Q: A 6.00 L tank at 17.4 °C is filled with 12.7 g of dinitrogen monoxide gas and 14.8 g of boron…

A: no. of moles = mass (g)molecular mass mole fraction = no of moles of one componenttotal moles given,…

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

A: We will first calculate the mole fraction of both O2 and N2 and then we will calculate the partial…

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…

A:

Q: Calculating partial pressure in a gas mixture A 8.00 L tank at 25.3 °C is filled with 4.35 g of…

A: Calculation  of mole fraction  of CO2 and N2F2 and partial pressure  and total pressure  of flask.

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…

A:

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…

A:

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: 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…

A:

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…

A:

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

A:

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: Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. R

A: Given: Volume= 30.0 L Pressure= 0.320 atm Temperature= 8.0oC= 281.15 K   To calculate:

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 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 8.00 L tank at 21. °C is filled with 4.85 g of sulfur tetrafluoride gas and 7.84 g of carbon…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 4.85 g Mass of carbon dioxide i.e CO2 = 7.84 g Volume…

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

A:

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 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 9.00 L tank at -3.4 °C is filled with 5.92 g of dinitrogen monoxide gas and 11.0 g of chlorine…

A:

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: 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 7.00 L tank at -5.1 °C is filled with 8.05 g of dinitrogen monoxide gas and 19.7 g of boron…

A:

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…

A:

Q: A 6.00 L tank at 14.6 °C is filled with 12.6 g of boron trifluoride gas and 5.55 g of sulfur…

A:

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

A: Answer:Dalton's law of partial pressure states that partial pressure of any gas in the gaseous…

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…

A:

Q: A 5.00 L tank at 11.4 °C is filled with 9.82 g of boron trifluoride gas and 11.4 g of sulfur…

A: A tank filled with boron trifluoride gas and sulfur hexafluoride gas. Given: weight of boron…

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…

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

A: Given: The number of N2 molecules present in the mixture is 7. The number of O2 molecules present in…

Q: A 8.00 L tank at 7. C is filled with 7.36 g of dinitrogen monoxide gas and 4.45 g of carbon monoxide…

A: Volume of tank = 8 LTemperature of tank = 7 0CAmount of dinitrogen monoxide gas = 7.36 gAmount of…

Q: A 8.00 L tank at 1.22 "C is filled with 9.39 g of sulfur tetrafluoride gas and 5.97 g of dinitrogen…

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

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.