Which of the following is NOT part of the kinetic theory of gases?     A. Gas particles do not attract or repel one another.     B. There is very little empty space in a gas.     C) Gas particles move faster when the temperature increases.     D. A gas is composed of very small particles.     E. Gas particles move rapidly.

Q: If the pressure is held constant, but the temperature of the gas inside a balloon is increased, what…

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Q: A sample of gas in a flexible container at room temperature exhibits a certain pressure. What will…

A: Answer: the new pressure will be the same old pressure. i.e P1=P2    Explanation: we know , P1-…

Q: Which statement about a closed, inflated, perfectly elastic balloon containing a given quantity of a…

A: The statement that is true about a closed, inflated, perfectly elastic balloon containing a given…

Q: The pressure and volume of a sample of gas are increased. What will happen to the temperature?…

A: According to the ideal gas equation, PVT=R where P is the pressure, V is the volume, T is the…

Q: Jacques Charles found that increasing the temperature of a gas sample at constant pressure would…

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Q: 9. Calculate the density of fluorine gas at STP. *diatomic gas*

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Q: A sample of xenon gas at a pressure of 1.04 atm and a temperature of 25.4° C, occupies a volume of…

A: Given, the initial pressure of xenon gas =1.04 atmat temperature =25.4 °Cinitial volume =18.1 Lnow…

Q: In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules…

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Q: Which of the following is an assumption made in the kinetic molecular theory of gases? Gas molecules…

A: Assumption of kinetic moleculer theory of gases:  1) Gases consist of large number of small…

Q: A student packs a suitcase full of clothes for an upcoming trip to Florida. The suitecase will not…

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Q: 1. According to the Kinetic Molecular Theory of Gases, which of the following would INCREASE the…

A: The concept used in this question is taken from kinetic molecular theory of Gases.  Now according to…

Q: Calculate the volume of each gas sample at STP. 1. 23.4  mol   Cl2 . 2. 3.9  mol  nitrogen. 3.2.6…

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Q: An iron nail rusts when exposed to oxygen. How many grams of iron are needed to completely consume…

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Q: What assumptions are made about the gas in the ideal gas equation model?  Consider Volume…

A: Since, we know that ideal gas equation PV = nRT  Where, P = pressure of gas  V= volume  T =…

Q: When the gas molecules escape to space it leaves the planet or the moon without?

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Q: An experiment, where the temperature was doubled and the pressure remained fixed, caused the gas…

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Q: n temperature.

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Q: If the mass of a proton is 1.007825 amu and the mass of a neutron is given as 1.008665 amu, If the…

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Q: The density of a gas at (STP ) is 1.17 g/L . What is the mass of the gas. Remember that the volume…

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Q: QUESTION 10 A bicycle tires filled in the summer feels flat when left till winter, with no one…

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Q: [References] Use the References to access important values if needed for this question. A sample of…

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Q: Use the References to access important values if needed for this question. A 7.33 gram sample of…

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Q: Samples of the gases listed below are all at the same temperature and volume. Which gas sample will…

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Q: which of the following gases will have the highest speed at room tempertaure?   A. hydrogen   B.…

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Q: Use the kinetic-molecular theory to explain the change in gaspressure that results from warming a…

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Q: Which of the following explains why decreasing the volume of a gas increases its pressure according…

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Q: neon

A: From ideal gas equation, we know that P1V1/ T1 = P2V2/ T2    ---------(i) Where, P1 = initial value…

Q: Which postulate best explains why gases are easily compressible? a. There are no attractive or…

A: To explain: To identify the postulate that best explains why gases are easily compressible.

Q: The graph below shows the relative speeds of various gases. at the same temperature. Select all true…

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Q: 1.42 mol sample of methane gas at a temperature of 7.00 degrees C is found to occupy volume of 21.6.…

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Q: Q1. Explain the ideal gas law using the molecular view of matter

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Q: A sample of gas is held at constant temperatures. if the pressure of gas in the sample is doubled…

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Q: One unit in R, when used in gas law calculations, that can NOT be changed is  A. oC B. L C. mm Hg…

A: R is a gas constant . Its value can vary depending upon the units used in your requirements.

Q: Avogadro's Law relates volume and amount of gas at a. constant temperature and pressure b. constant…

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Q: How are pressure , volume in gasses related?

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Q: 27. How will the volume of a fixed sample of gas change if its pressure is doubled and the Kelvin…

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Q: According to the kinetic molecular theory, which of the following is true? Select all that apply.…

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Q: Which of the following properties describes a gas? O A. Have a fixed shape and volume. O B. High…

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Q: Which of the following statements regarding the density of gases is NOT correct? A)The density of a…

A: Given statements, A) The density of a gas is inversely proportional to its molar mass. B) As the…

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.