A 15.0 L tank is filled with helium to a pressure of 2.00 * 10^2 atm. How many 2.00 L balloons can be inflated to a pressure of 1.00 atm from the tank. Assume that there is no temperature change and that the tank cannot be emptied below 1.00 atm. (I don't understand. Could you show me step by step please?)

Q: What mass of neon gas would be required to fill a 3.00-L flask to a pressure of 925 mm Hg at 26 °C?

A: Ideal Gas Law :-  PV = nRT  P is the pressure of gas  V is the volume occupied by gas n is the…

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A: a)Plot of volume ( x-axis) versus 1/pressure (y-axis) is given below.

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Q: A helium balloon at sea level has a volume of 2.10 L at 0.998 atm and 36.1oC. If it is released and…

A: Given: V1=2.10 L P1=0.998 atm. V2=? P2=0.900 atm

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A:

Q: 70. What mass of neon gas would be required to fill a 3.00-L flask to a pressure of 925 mm Hg at 26…

A: PV = nR T  where  P = 925 mm Hg x 1 atm/760 mmHg = 1.217 atm V = 3 L T = 26 °C = 26 + 273 K = 299 K…

Q: A sample of air occupies 2.50 L at a temperature of 22.0 oC. What volume will this sample occupy…

A: Here i have solved via charle's law

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A: Given for argon gas P1 = 0.924 atm T1 = 20.2 °C = (20.2 + 273)K = 293.2 K V1 = 437 mL Temperature is…

Q: A sample of a refrigeration gas in a volume of 458 mL, at a pressure of 1.10 atm, and at a…

A: Conditions before compression,V1 = 458 mL = 0.458 LP1 = 1.10 atmT1 = 12oC = 12 + 273.15 =…

Q: The atmospheric pressure on Mount Logan in the Yukon is 520. mbar. What is the pressure in torr?…

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Q: A 250.0-mL sample of ammonia, NH3(g), exerts a pressure of 833 torr at 42.4°C. What mass of ammonia…

A: The can be calculated from the known values of molar mass and no of moles. Mass=molar mass×no of…

Q: A sample of ammonia (NH3), a colorless gas with a pungent odor, occupies a volume of 9.00 L at a…

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A: Mass of carbon dioxide = 25.0 g

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A:

Q: 1. If 23.0 L of nitrogen at 780 mm Hg are compressed to 730 mm Hg at constant temperature. What will…

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A: T1=281°C=(281+273)K=554K V2=448mL=0.448L V2=339mL=0.339L T2=?

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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 volume of a sample of hydrogen gas was decreased from 12.36 L to 5.65 L at constant temperature.…

A: Given: The initial volume, of hydrogen gas (V1) = 12.36 L. The final volume, of hydrogen gas (V2) =…

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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

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Q: The volume of a sample of hydrogen gas was decreased from 13.77 L13.77 L to 7.06 L7.06 L at constant…

A: As per the given data we haveInitial volume (V1)=13.77LFinal Volume (V2)=7.06LFinal pressure…

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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…

A: Given information:Mass of dry ice = 1.20 gVolume of flask  = 765 mLPressure = 725 mmHgTemperature =…

Q: A sample of ammonia (NH3), a colorless gas with a pungent odor, occupies a volume of 7.00 L at a…

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Q: A flask contains a mixture of oxygen, nitrogen, and hydrogen gases. If the partial pressure of…

A: • The values provided in the question are:-    i) Partial pressure of oxygen gas, PO2 = 546. 0 mm Hg…

Q: 1. A 2.5 L container has a gas pressure of 4.6 atm. If the volume is decreased to 1.6 L, what will…

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Q: A 16.0 L sample of chlorine gas has a pressure of 28.0 atm at a certain temperature. At the same…

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Q: 11) The temperature of a 9382 mL sample of Ne is changed, causing a change in pressure from 121.94…

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Q: A sample of ammonia (NH3), a colorless gas with a pungent odor, occupies a volume of 3.00 L at a…

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Q: A 10.5 L balloon contains helium gas at a pressure of 655 mmHg. What is the final pressure, in…

A: GivenVolume of ballon = V = 10.5 LPressure of ballon = P =  655 mmHg

Q: A 20.0-L tank contains 0.486 g of helium at 18 deg C. The molar mass of helium is 4.00 g/mol. What…

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Q: Oxygen gas is commonly sold in in 49.0 L steel containers at a pressure of 150 atm. What volume in L…

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Q: A piece of dry ice (solid carbon dioxide) with a mass of 25.5 g sublimes (converts from solid to…

A: According to ideal gas equation,  PV = nRT V = (nRT÷P) n = moles = (given mass ÷ molecular mass)

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.