What is a real gas, and how does it relate to the kinetic molecular theory? Explain how two assumptions of the theory are not followed by a real gas.

Q: A balloon is filled with helium gas (see an illustration below). Indicate whether the volume of the…

A: A balloon is filled with helium gas (see an illustration below). Indicate whether the volume of the…

Q: A mixture of gases contained only three types of gases (Ne, Ar and He) has a total pressure of 0.900…

A: Given:Mole fraction of Ne = 0.36Mole fraction of Ar = 0.44Total pressure = 0.9 atm.

Q: A sample of argon gas occupies a volume of 6.03 L at 58°C and 446 mm Hg. The volume of the gas…

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Q: to form Cl2 and NaF. Use the ideal gas law equation to determine the mass of NaCl that reacted with…

A: Given :  Volume = 15.0 L Pressure = 1.50 atm  Temperature = 280 K R = 0.082 L.atm/mol.K Moles = ?…

Q: A high-altitude balloon contains 30.0 L of helium gas at 1.00 kPa. When the balloon moves to an…

A: Given data---> V1=30.0 L P1= 1.00 kPa P2= 25.0 kPa V2= ?

Q: 1. A sample of gas weighs 3.10 g and occupies a volume of 1,272 mL at 30 °C and 720 mm Hg. What is…

A: According to ideal gas law, PV = nRT where P = pressure in atm  V = volume in L n = moles R = gas…

Q: What mass of helium gas is present in a 10.3-L sample of this mixture at 283 K ?

A: Given a gas mixture of CO2 , Ar, O2 and He gases with total pressure =770 mmHg and partial pressure…

Q: partial pressure in a gas mixture sulfur tetrafluoride A 8.00 L tank at 29.8 °C is filled with 14.2…

A: The ideal gas equation is a fundamental equation in thermodynamics that describes the behavior of…

Q: How does Dalton's law of partial pressures help us with our model of ideal gases? That is, what…

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Q: occupies

A: Ideal gas equation, PV = nRT  Temperature is constant  PV = constant  For, initial condition : P1V1…

Q: What two gas variables are kept constant in a Boyle’s law experiment?

A: Boyle's lawAccording to the Boyle's law as the pressure (P) increases the volume (V) of a gas…

Q: A pressurized gas is allowed to expand.  If the gas originally occupied a volume of 420 mL at a…

A: The question is based on the concept of Boyle's law.   it states that for a given amount of gas , at…

Q: 13.) A 1.75 gram sample of an unknown gas is found to occupy a volume of 1.24 L at a pressure of 624…

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Q: For carbon dioxide the numerical value of a  is  3.592  and the numerical value of  b  is…

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Q: At 25 °C, a gas occupies a volume of 1.20 L under 0.295 atm of pressure. At what temperature will…

A: According to ideal gas equationThe number of moles can be calculated as

Q: The Ideal Gas Law cannot be manipulated. O True O False

A: Ans.  The Ideal Gas Law is very simply and can be expressed as  PV = nRT  The equation has four gas…

Q: Calculate the pressure of a 14.6 L container with 60.6 moles of hydrogen, at -14.5 degree C,…

A: The volume of container is 14.6 L. The number of moles of hydrogen gas is 60.6 mol. The value of…

Q: the kinetic Match the characteristic of gases described below to the postulates of molecular theory…

A: 1) The Kelvin temperature is exactly proportional to the pressure of a certain volume of gas kept at…

Q: Which of the following statements is (are) true? a. If the number of moles of a gas is doubled, the…

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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.