Graham's Law: If 2.2x10-4 mol N2(g) effuses through a tiny hole in 105 s, then how much O2(g) would effuse through the same orifice in 105 s?

Q: At a given temperature and pressure, it takes 9.48 minutes for a 1.5 L sample of He to effuse…

A: In this question, we want to determine the time for F2 effuse under given temperature and pressure.…

Q: A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 667 torr. Use…

A: Given, Initial volume Vi=10.0 L Initial pressure, Pi= 667 torr Final volume, Vf=8.13 L Final…

Q: A sample of gas is manipulated so that its temperature (in K) triples and its volume is reduced to…

A: An ideal gas will follow the ideal gas equation. The ideal gas equation is given by PV=nRT, where P,…

Q: 5.A gas of unknown molecular mass was allowed to effuse through a small opening under constant…

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Q: A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.24 L1.24 L was placed in a weighted…

A: According to Boyle's Law, at constant temperature the volume of given amount of gas is inversely…

Q: A 6.96 gram sample of an unknown gas is found to occupy a volume of 2.10 L at a pressure of 912 mmHg…

A: Given that: mass of sample = 6.96 g volume of gas = 2.10 L pressure of gas = 912 mmHg temperature =…

Q: A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.62 L1.62 L was placed in a weighted…

A: Given: Initial Pressure, P1 = 1.00 atm Initial volume, V1 = 1.62 L Final Pressure, P2 = 80.0 atm…

Q: Given that 7.10 moles of carbon monoxide gas are present in a container of volume 29.8 L, what is…

A: Given values are, n= 7.10 mol V= 29.8 L T=55°C= 328.5 K Standard value, Gas constant R= 0.08205…

Q: What pressure does the gas exert if the temperature changes from T1 = 600. K to T1 = 300. K, while…

A: According to Gay-Lussac's law, at constant volume pressure increases, temperature increases.

Q: According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K…

A: The objective of the question is to calculate the percent difference between the pressure calculated…

Q: Use the van der Waal's Equation to calculate the pressure exerted by 80.0 grams of hydrogen sulfide…

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Q: A 7.94 g piece of solid CO 2 (dry ice) is allowed to sublime in a balloon. The final volume of the…

A: Given: mass of CO2 = 7.94 g Volume of balloon = 1.00 L Temperature = 301 K molar mass of CO2 = 44.01…

Q: A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.72 L1.72 L was placed in a weighted…

A: According to Boyle’s law At constant Temp. P1V1 = P2V2 P1 = 1atm        P2 = 65atm V1 = 1.72 L    V2…

Q: A sample of O2 gas is observed to effuse through a porous barrier in 7.64 minutes. Under the same…

A: Effusion is the process of movement of gaseous molecules through a small hole. The rate of effusion…

Q: A sample of SO2 gas is observed to effuse through a porous barrier in 5.45 minutes. Under the same…

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Q: What pressure will be exerted by 0.7 mol of a gas at 23 °C when contained in a vessel whose volume…

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Q: According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K…

A: To calculate the percent difference between the pressure predicted by the ideal gas law and the…

Q: If 0.150 mol of N2 gas effuses through a small hole over the course of one hour, calculate the…

A: Given: Molar mass of H2 gas = 2.0158 g / mol Molar mass of N2 gas = 28.01 g / mol

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.