Perform the conversions. 463.1 mmHg = 0.6093 143.8 kPa = atm atm 1.388 atm = 1075.4 mmHg = Torr Pa

Q: Convert the following 34.5 atm= mmHg 30.39 kPa= torr

A: We have given that 34.5atm =                mmHg 30.39kPa =                 torr

Q: Calculate the final temperature of a sample of gas initially at 22.3 0C that is expanding from 2.335…

A: As per the ideal gas law, PV = nRT  where P = pressure  V = volume  n = moles  R = gas constant  T =…

Q: A gas occupies 3.33 L at STP. What pressure in Torr will this gas exert if it is expanded to 7.47 L…

A: Given that, in first condition: The volume of gas (V1) = 3.33 L, at STP conditions. For STP, the…

Q: Convert 747.6 mmhg to atm

A: 1 atm = 760 mm Hg  Thos conversion factor will be used to convert mm Hg to atm

Q: Convert 836 Torr to atmospheres. 836 Torr = Convert 27.0 atm to torr. 27.0 atm = Convert 836 mmHg to…

A: The objective of the question is to convert the given values from one unit of pressure to another.…

Q: convert 680 torr to kPa

A: convert 680 torr to kPa

Q: -5 atm to kPa 50 atm to bar -937 kPa to torr

A: Answer 1)    76cm Hg is equal to                 =  1 atm  then ,  76.8cm Hg is equal to = (76.8 ×…

Q: A balloon is filled to a volume of 1.50 L with 3.00 moles of gas at 25.0 °C. With pressure and…

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Q: Convert 2.68 atm to cm Hg

A: 1 atm = 76 cm hg

Q: A bulb contains 3.894 g of He at a temperature of 17.4 oC and a pressure of 759.3 torr.  Determine…

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Q: The volume of a gas ends up being 40.1 L. The change occurred because the pressure was changed from…

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Q: A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mm Hg and a temperature of…

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

Q: If you pack a bag of potato chips for a snack on a plane ride, the bag appears to have inflated when…

A: Given :-  Initial pressure = 760 mm Hg  Initial volume = 340 mL  Final pressure = 670 mm Hg  To…

Q: A gas originally occupying 10.1L at 0.925 ATM and 25 degrees is changed to 13.3 L at 625 torr. What…

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Q: A gas that has a volume of 26.3 L, a temperature of 58.3°C, and an unknown pressure has its volume…

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Q: balloon is filled to a volume of 1.50 L with 3.00 moles of gas at 25.0 °C. With

A: Here we have to use the gas equation PV=nRT Here P and T are constant so V directly proportional to…

Q: A sample of a gas occupies a volume of 29.6 L at 16 ºC and 614 torr. What will be the new volume if…

A: Intial volume  = V1 = 29.6 L  Intial temperature = 16 ºC.     ( 0 °C = 273.15 K ) Intial temperature…

Q: What is the mass of CO2 that occupies 14.5 L at 455mmHg and 45.5 degrees Celsius

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Q: Convert each pressure unit to the indicated unit. Remember to use the correct number of significant…

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Q: convert 680 torr to mmHg

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Q: Convert 797 mmHg to atm.

A: Since 1 atm = 760 mm Hg

Q: If a gas at 25.0°C occupies 2.75 liters at a pressure of 1.04 atm, what will be its volume at a…

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Q: Convert 11 atm to mmHg.

A: Given 1 atm= 770mm of Hg 11 atm=?

Q: Convert 18.15 psi to mmHg. Provide an answer with TWO decimals. Your Answer:

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Q: A balloon has a volume of 0.855 L at 1.0 atm and 17.0 degrees celcius. If the pressure remains…

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Q: 921 torr to atm   340. kPa to atm    750. mmHg to kPa

A: Conversion of pressure measurements--

Q: If 2.00 L of gas at 20.0 degrees C and 760 mm Hg is allowed to come to 245 mmHg at 350.0°C, what is…

A: In this question ideal gas equation is used. Since number of moles is constant so, PV/T = constant

Q: 2.50 mol of a gas at 10 degrees Celsius occupies 55.5 L.  Determine the pressure of the gas. - 106…

A: Given-> Mole of gas = 2.50 mole Temperature = 10°C = 10+273 = 283K  Volume= 55.5 L

Q: Convert 459.06   mmHg to torr

A: Given, Convert 459.06 mmHg to torr Note: Here, we have units of pressure and we know that, 1 mmHg =…

Q: A sample of gas has a volume of 4.54 L at 24.4 ∘C and 749 mmHg. What will be the volume of this gas…

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Q: A sample of gas has a volume of 2.22 L at 0.995 atm and 35.0°C. What is the pressure (in atm) of the…

A: According to the Ideal gas equation: P1V1T1=P2V2T2......(1) Where, P is the pressure. T is the…

Q: Convert 0.955 atm to mm Hg

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

Q: A gas sample is confined to 3.0L and kept at 27.0 Celsius. If the temperature is raised to 93…

A: The given data contains,  volume = 3 L. Temperature T1 = 27°C Temperature T2 = 93°C Pressure P1 =…

Q: Using the following equalities and the relationships between atm and torr or mmHg you are required…

A: we know that 1.00 atm = 29.92 inHg

Q: Calculate the final pressure of a gas in atm that was initially occupying 51.22 cm3 at 865.45 mmHg…

A: Given  Initial Volume ( V1 )  = 51.22 cm3                                   = 51.22 mL…

Q: Convert each of the following into the desired units. 790mmHg to atm

A: We have given that  790mmHg to atm  We know that  mmHg and atm are the unit of Pressure   Pressure =…

Q: If a sample of carbon dioxide gas in a 455.0 ml container has a pressure of 725.0 mmHg at -49.0oC,…

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Q: A mixture of helium and neon gases has a density of 0.240 g/L at 41.0°C and 382 torr. Find the mole…

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Q: A sealed balloon is filled with 1.00 L helium at 21°C and 1.00 atm. The balloon rises to a point in…

A: By combining the three gas laws, namely Boyle’s Law, Charle’s Law and Avogadro’s Law, a combined gas…

Q: A 841 mL sample of NH3 gas is at STP. If the volume changes to 576 mL and the temperature changes to…

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Q: What is the mass of 12.0L of Chlorine gas (Cl2, 70.9 g/mol) measured at 1250mmHg and 157C? a) 2.94…

A: We have 12 L of Cl2 gas measured at pressure of 1250 mmHg and 157°C. We have to calculate the mass…

Q: The partial pressure of carbon dioxide in the atmosphere is 0.000314 atm. Calculate the partial…

A: The partial pressure of carbon dioxide in the atmosphere is 0.000314 atm. We have to calculate the…

Q: A balloon is filled to a volume of 1.50 L with 3.00 moles of gas at 25.0 °C. With pressure and…

A:

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.