A balloon is filled with helium gas to a volume of 2.5 L at a pressure of 99.6 kPa and a temperature of 24 °C. What Gas Law am I using if I decide to keep the pressure of the gas constant, and I manipulate the temperature to find the new volume of the gas? Ideal Gas Law Boyle's Law Combination Law Charles's Law Gay-Lussacs

Q: A 8.00 L tank at 1.27 °C is filled with 9.88 g of dinitrogen difluoride gas and 13.1 g of chlorine…

A: GivenMass of dinitrogen difluoride gas = 9.88 gmolar mass of dinitrogen difluoride gas = 66.010…

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 6.00 L tank at 12.2 °C is filled with 5.23 g of chlorine pentafluoride gas and 13.7 g of boron…

A: Ideal gas equation:  PV = nRT  P = Pressure V = Volume n = Total number of moles  R = Gas constant T…

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: Consider a sample of air in a sealed container. Explain how the pressure of a gas would be affected…

A: 1) According to ideal gas law, PV = nRT where P = pressure V = volume n = moles R = gas constant T =…

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

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Q: A cylinder is filled with 10.0L of gas and a piston is put into it. The initial pressure of the gas…

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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: 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: A 10.0 L tank at 0.86 °C is filled with 12.3 g of dinitrogen difluoride gas and 9.28 g of chlorine…

A: According to the question, The temperature of the tank is = T= 0.86°C = 273.15+0.86 K = 274.01 K The…

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 mixture of 34.23 moles of argon, 12.76 moles helium, 21.53 moles neon, and 42.33 moles krypton is…

A: Given : Volume of vessel = 2935.34 L Moles of Argon =  34.23 moles Moles of Helium= 12.76 moles…

Q: A 5.00 L tank at 4.58 °C is filled with 15.2 g of chlorine pentafluoride gas and 7.62 g of sulfur…

A: Ideal gas equation: PV = nRT  P = Pressure V = Volume n = Number of moles  R = Gas constant T =…

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…

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Q: A 7.00 L tank at 9.47 °C is filled with 6.90 g of dinitrogen difluoride gas and 5.31 g of chlorine…

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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 sample of nitrogen gas has a volume of 478 cm³ and a pressure of 104.1 kPa. What volume would the…

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Q: A 9.00 L tank at 28.9 °C is filled with 8.24 g of sulfur tetrafluoride gas and 5.83 g of chlorine…

A: Volume of the tank = 9 LTemperature = 28.9 0CAmount of sulfur tetrafluoride = 8.24 gAmount of…

Q: A mixture of 30.74 moles of argon, 13.1 moles helium, 20.59 moles neon, and 42.99 moles krypton is…

A: Given data  T = 141.83 °C V= 2792.92 L  Number of moles are given of different gases

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: 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: Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle’s Law is described…

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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: 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…

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Q: 10.0L

A: We will use Boyle's law

Q: A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas…

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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: A 1.62-mol sample of methane gas is maintained in a 0.660-L container at 305K. Calculate the…

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Q: Hydrogen gas, oxygen gas, and water vapor are collected in eudiometer. The eudiometer contains…

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Q: A sample of gas contains 4.19 moles at 37.8 °C in a volume of 3.61 L. If 2.67 moles of gas are…

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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 6.00 L tank at 7.28 °C is filled with 9.73 g of sulfur tetrafluoride gas and 2.46 g of carbon…

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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 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: 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: A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen…

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Q: A 9.00 L tank at 1.5 °C is filled with 3.22 g of carbon monoxide gas and 16.7 g of chlorine…

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Q: 92  and the numerical value of  b  is  0.0429 .   Use the van der Waals equation to calculate…

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Q: A gas mixture with a total pressure of 765 mmHg contains each of the following gases at the…

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Q: A 8.00 L tank at 24.8 °C is filled with 4.16 g of chlorine pentafluoride gas and 11.6 g of sulfur…

A: The mass of Chlorine pentafluoride, ClF5 = 4.16 gThe mass of Sulfur hexafluoride, SF6 = 11.6 gThe…

Q: A sample of helium gas occupies a volume of 8.64 L at 41.0°C and 0.960 atm. If it is desired to…

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Q: A 9.00 L tank at 7.61 °C is filled with 9.76 g of sulfur hexafluoride gas and 6.26 g of chlorine…

A: we have to calculate mole fraction, partial pressure of each gas and the total pressure in the tank

Q: A 7.00 L tank at 5.4 °C is filled with 3.81 g of sulfur tetrafluoride gas and 11.1 g of dinitrogen…

A: Ideal gas equation is  PV = nRT  Where,  P is pressure of the gas  V is volume n is no. of moles  R…

Q: A 9.00 L tank at 9.4 °C is filled with 10.7 g of dinitrogen monoxide gas and 13.1 g of carbon…

A: The mole fraction of a component in the mixture is defined by the ratio of moles of that substance…

Q: A sample of gas has a volume of 2.50 L at 651 kPa and 75.0 °C. What is the pressure (in atm) of the…

A: Answer:When number of moles of the gas is constant then ideal gas law for a gas is:Here:

Q: 6.00 L tank at 27.2 °C is filled with 4.10 g of chlorine pentafluoride gas and 8.51 g of boron…

A:

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.