If 28.8 g of O₂ is required to inflate a balloon to a certain size at 32.0 °C, what mass of O₂ is required to inflate it to the same size (and pressure) at 9.0 °C? Mass= g

Q: For many purposes we can treat methane (CH4) as an ideal gas at temperatures above its boiling point…

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Q: A sample of an ideal gas at 1.00 atm and a volume of 1.09 I was placed in a weighted balloon and…

A: To find out the new volume of an ideal gas, use the formula of Boyle's law and find out the volume…

Q: A mixture of methane and xenon gases is maintained in a 6.38 L flask at a temperature of 79°C. If…

A: Given data : Volume of the flask = 6.38 L Temperature = 79°C Partial pressure of methaneP1=0.423 atm…

Q: The maximum safe pressure that a certain 4.00-L vessel can hold is 3.21 atm.  If the vessel contains…

A: The temperature, pressure, volume, and mole of the gas are related by the ideal gas equation. The…

Q: What is the temperature, in degrees celcius, of 1.50 moles of neon (Ne) gas confined to a volume of…

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Q: Calculate the change in volume of a 3.26 L sample of Argon, at 0.999 atm, that is heated from 22 oC…

A: Given data, Initial volume(V1)=3.26LInitial pressure(P1)=0.999atmInitial…

Q: example in Part A has an initial volume of 42.0 L , and you have determined that it contains 1.60…

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Q: None

A: Step 1Determine the volume of the flask using the mass of water and the density of water at 18.0∘C.…

Q: A sample of an unknown compound is vaporized at 150.°C. The gas produced has a volume of 510.mL at a…

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Q: A steel cylinder contains 150.0 moles of argon gas at a temperature of 25°C and a pressure of 8.93 M…

A: Answer:- This question is answered by using the simple concept of ideal gas equation which involves…

Q: An ideal gas in a sealed container has an initial volume of 2.80 L. At constant pressure, it is…

A: At constant pressure and amount, the combined gas law states that: V1T1=V2T2    ............... (1)…

Q: A typical barometric pressure in Denver, Colorado, is 610.2 mm Hg. What is this pressure in…

A: In order to convert the pressure from millimeters of mercury (mm Hg) to atmospheres (atm), we need…

Q: If 13.9 g of O₂ is required to inflate a balloon to a certain size at 36.0 °C, what mass of O2 is…

A: The relationship between the temperature, pressure, and volume of the initial and final state of an…

Q: 4. A light bulb contains 0.0560 g of Argon gas with a pressure of 1.34 atm at 26.0 °C. The light…

A: Ideal gas equation can be used to calculate P, V, T and number of moles of ideal gas:    P×V=n×R×T…

Q: A gas has the initial conditions of: 21.2 Liters 279 K 1.03 atmospheres If its pressure is increased…

A: We are authorized to answer one question at a time, since you have not mentioned which question you…

Q: A sample of solid potassium chlorate was heated in a test tube and decomposed into potassium…

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Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

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Q: A metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and…

A: Given: Volume = 6.0 L Initial pressure of cylinder = 120 atm Initial temperature of cylinder =  75…

Q: A 2.50 gm sample of liquid ether is placed in a 1.50-L flask and vaporized by heating to 75°C at…

A: From ideal gas equation PV=nRT , by using giving information we can find molar mass.

Q: You purchase a butane tank that can hold gas safely up to a pressure of 38.7 atm. When the tank…

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Q: A 1.20 g sample of dry ice is added to a 765 mL flask containing nitrogen gas at a temperature of 25…

A: We have to calculate the total pressure inside flask .

Q: Humidity is the percentage of partial pressure of water in air over the total possible water in the…

A: Introduction Humidity is an important concept in chemistry. It refers to the amount of water vapor…

Q: 4. A sample of hydrogen is collected by displacing a sample of water with a temperature of 35°C. The…

A: Given Total pressure of mixture = 114 kPa

Q: For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point…

A: The Ideal Gas equation is given by,PV = nRTwhere,P= Pressure in atmV = Volume in LT = Temperature in…

Q: A 0.790 g sample of an unknown substance was vaporized in a 250. mL flask at 77.1 °C and 1.03 atm.…

A: Since the sample is finally in gaseous form. Hence the ideal gas law is applicable. According to…

Q: A sample of helium gas occupies a volume of 9.12 L at 54.0°C and 0.640 atm. If it is desired to…

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Q: For many purposes we can treat propane (C3H8) as an ideal gas at temperatures above its boiling…

A: Given: The initial pressure = 4.2 atm The initial temperature = -22.0 oC The final temperature =…

Q: For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point…

A: Answer: This question is based on ideal gas equation where we have to calculate the value of new…

Q: What mass of helium gas is needed to pressurize a 92.0 L tank to 209 atm at 18 °C? What mass of…

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Q: 6. Determine the total pressure exerted by a mixture of 2.00 g hydrogen gas and 8.00 g of nitrogen…

A: Dalton's Law of partial pressure: The total pressure exerted by a mixture of gas is equal to the sum…

Q: A 1.07 g sample of a liquid is evaporated completely at 341 K so that its vapors fill a 0.252L…

A: A 1.07 g sample of a liquid is evaporated completely at 341 K so that its vapors fill a 0.252 L…

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: A sample of krypton at 38.5 °C had a pressure of 0.710 atm. When the pressure changed to 0.851 atm…

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Q: Another balloon is inflated to a volume of 1.250 L with dry hydrogen gas, at 28.0 °C. The balloon is…

A: Here, pressure is constant during the process.  Hence, Chales law is applicable

Q: A sample contianing 6.88g of solid CO2 is put in an empty sealed 5.4L container at a temperature of…

A: Using ideal gas equation  PV = nRT Where P is the pressure  V is the volume  R is the gas constant =…

Q: A mixture of He, Ne, and Ar has a pressure of 28.2 atm at 28.0 °C. If the partial pressure of He is…

A: Total Pressure of mixture is represented as,

Q: Calculate the pressure in a sealed 4.00 L flask that contains 56.3 g O2 (MM = 32.00g/mol) at 30.0…

A: The ideal gas equation describes the relationship between different parameters of a gas. These…

Q: the change in volume of a 3.26 L sample of Argon, at 0.999 atm, that is heated from 22 oC to 35o C…

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Q: A 27.1 g sample of solid CO2 (dry ice) is added to a container at a temperature of 100 K with a…

A: When the temperature is increased from 100K to 298K, CO2 will be in the gaseous phase but mass, and…

Q: For many purposes we can treat nitrogen (N2) as an ideal gas at temperatures above its boiling point…

A: We have Initial temperature = T1 =  –88 °C = –88 + 273 = 185 K Initial pressure = P1 = P Initial…

Q: A sample of He(g) at 27 °C and 0.95 atm is heated in a constant volume container to a new pressure…

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Q: The volume of H2O2 give was 5.00 mL. The temperature is 21.4 C. Suppose the gas that was collected…

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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.