A sample of He gas is observed to effuse through a pourous barrier in 5.26 minutes. Under the same conditions, the same number of moles of an unknown gas requires 17.1 minutes to effuse through the same barrier. What is the molar mass of the unknown gas

Q: At a given temperature and pressure, it takes 9.48 minutes for a 1.5 L sample of He to effuse…

A: In this question, we want to determine the time for F2 effuse under given temperature and pressure.…

Q: . A gas occupying a volume of 528 ml at a pressure of 745 mmHg and at a temperature of 12 ° C, was…

A: To solve this problem we will use combined gas law which is  P1V1/T1 = P2V2/T2   Where ,…

Q: if 0.3781 g of a gas with a molecular weight of 18.015 g/mol is in a ridged 5.00 l container at 384…

A: The ideal gas equation for the relation between pressure (P), volume (V) and temperature (T)…

Q: A 7.00 L tank at -6.3 °C is filled with 18.4 g of dinitrogen difluoride gas and 4.58 g of dinitrogen…

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Q: Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the…

A:

Q: What volume is occupied by a 0.978 mol sample of oxygen gas at a temperature of 0 °C and a pressure…

A: To determine the volume occupied by a sample of oxygen gas, we can use the ideal gas law…

Q: A sample of Helium gas is observed to effuse through a pourous barrier in 5.26 minutes. Under the…

A: Given, effusion time He gas =5.26 minuteseffusion time of unknown gas =17.1 minutesboth the gas has…

Q: A 1.92 gram sample of an unknown gas is found to occupy a volume of 1.19 L at a pressure of 599 mmHg…

A: PV = nRT n = Mass/molar mass

Q: CO2 effuses 1.42 times more rapidly than the unknown gas. What is the molar mass of the unknown gas?

A:

Q: For a 0.00554 mol sample of H2 and a 0.00912 mol sample of N2, total pressure is 23.44 torr. What is…

A: Given, moles of H2 = 0.00554 moles Moles of N2 = 0.00912 moles Total pressure, pT = 23.44 torr

Q: The mole fraction of Nitrogen in air is 0.14 and the mole fraction of Oxygen in air is 0.66…

A: Pressure of room( Ptotal) = 1 atm (standard atmospheric pressure) mole fraction of Oxygen in…

Q: A mixture of gases containing 0.362 moles of oxygen, 1.23 moles of nitrogen, and 0.0234 moles of…

A: Given: moles of O2 = 0.362 mol moles of N2 = 1.23 mol moles of Ar = 0.0234 mol Total pressure = 2.60…

Q: A gas made up of atoms escapes through a pinhole 2.04 times as fast as Kr gas. Write the chemical…

A:

Q: 1.50 grams of nitrogen (N₂) gas is sealed in a 750.00 ml container at 35.0°C. Calculate the pressure…

A:

Q: At what temperature does 0.027325 moles of Ne in a 998.2 mL container exert a pressure of 0.813 atm?

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

Q: 1) 27 L of CO2 is initially collected at 299K. After, the temperature is increased to 323 K.…

A:

Q: A mixture contains O2 at 700. torr pressure, F2 at 900. torr pressure, and Cl2 at 400. torr…

A: Given that, Pressure of O2=700 torr pressure of F2=900 torr pressure of Cl2=400torr then,

Q: Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through…

A:

Q: Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through…

A: To Calculate molar mass of unknown gas , we would use the relation between rate of effusion and…

Q: the same barrier. The molar mass of the unknown gas is ____g/mol.

A: We have to find molar mass of the unknown gas

Q: 2.58 gram sample of an unknown gas is found to occupy a volume of 1.53 L at a pressure of 687 mmHg…

A: Given that:  Mass of gas = 2.58g Volume(V) = 1.53L P = 687 mmHg = 687mmHg×1atm/760mmHg = 0.9039atm T…

Q: partial pressure

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Q: A 2.0 L flask contains 0.363 g of nitrogen gas and 0.796 g of carbon monoxide gas. What is the mole…

A: Number of mols of N2 = given mass / molar mass = 0.363 g / 28.0134 g/mole = 0.129 moleNumber of mols…

Q: Imagine that you have a 6.50 LL gas tank and a 4.50 LL gas tank. You need to fill one tank with…

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Q: and gas B has a molar mass of 24.28 g. If each gas is introduced at the opposite end of a 1.5 m…

A: Graham's law of diffusion states that the rate of diffusion of a gas is inversely proportional to…

Q: Gas Y effuses half as fast as O2. What is the molar mass of gas Y?

A: rate of effuses is inversely proportional to the square root of the molar mass of gas.

Q: Determine the total pressure exerted by a mixture containing two gases if the partial pressure of…

A: Given that, P1 = 70 atm P2= 30 atm PT= ?

Q: A mixture of 0.500 mol of Ne and 0.250 mol Ar have a total pressure of 3.20 atm. What is the partial…

A:

Q: A sample of Kr gas is observed to effuse through a porous barrier in 5.98 minutes. Under the same…

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Q: A 0.916 gram sample of an unknown gas is found to occupy a volume of 0.789 L at a pressure of 515 mm…

A:

Q: A sample was collected and analyzed. If there are only three gasses present, the total pressure of…

A: Pressure of Nitrogen (pN2) = 74.17 kPa Pressure of Oxygen (pO2) = 7.88 kPa Pressure of Fluorine…

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.