Which of the following samples has the most moles of gas? O 1.90 Lof CH4 gas at 25 °C and 760 mm Hg O 1.00 Lof Cl, gas at 25 °C and 760 mm Hg O 3.50 Lof NH3 gas at 25 0C and 760 mm Hg O 6.20 Lof Ar gas at 25 °C and 760 mm Hg O 0.30 Lof O, gas 25 °C and 760 mm Hg

Q: A sample contains 2.0 moles of He gas and 6.0 moles of Ar gas. What is the mole fraction of He gas…

A: The mole fraction of a component in the mixture is defined by the ratio of moles of that substance…

Q: At 2°C a 1.0-L flask contains 1.0x 10^-2  mole of N2 , 4.0x10^2 mg O2 , and 5.1x 10^21 molecules of…

A: N2 =  1.0x 10^-2  mole = 0.01 mole O2 =  4.0x10^2 mg =400 mg =0.4 g O2 = 0.4 g / 32g/mol = 0.0125…

Q: 69. The partial pressure of CH4(g) is 0.175 atm and that of O,(g) is 0.250 atm in a mixture of the…

A: Please find the solution below:

Q: A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a…

A: Given,  90.0% CH4, 8.9% C2H6, and 1.1% C3H8.Total pressure of 307.2 kPa.Partial pressure is…

Q: 14)a) A sample of neon gas occupies a volume of 50.00L at 27.00C and 10.0 atm. How many moles of…

A:

Q: Two bulbs are connected by a stopcock. The large bulb, with a volume of 6.00 L, contains nitric…

A: Given: The volume of the large bulb = 6.00 L The pressure of the large bulb = 0.750 atm The volume…

Q: 1. A mixture of 1.00 g of Hzand 1.00g of He is placed in a 1.00L container at 27C. Calculate the…

A: Since you have posted multiple question. We will solve the first question for you. To get the…

Q: 165mL of gas is compressed to 43mL If the original pressure was 6 atm and the temperature is held…

A:

Q: Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: •Given:-

Q: A container of O2 gas at 75 °C has a volume of 3.5 liters at 1.3 atm. What is the new volume of the…

A: Given :-  Initial pressure (P1) = 1.3 atm  Initial volume (V1) = 3.5 L Final pressure (P2) = 0.80…

Q: partial pressure in a gas mixture sulfur tetrafluoride A 8.00 L tank at 29.8 °C is filled with 14.2…

A: The ideal gas equation is a fundamental equation in thermodynamics that describes the behavior of…

Q: A mixture of two gases with a total pressure of 5.20 atm contains 1.50 atm of Gas A. What is the…

A: we have to calculate the partial pressure of gas B

Q: A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a…

A:

Q: A gas exerts a pressure of 1atm at standard temperature. What should be the new temperature (in…

A:

Q: 3a. Write down the two versions of the Ideal Gas Law and define each term and its units. 3b. How…

A:

Q: A 10.00 L tank at 29.5 °C is filled with 5.59 g of sulfur tetrafluoride gas and 12.5 g of carbon…

A: mass of Carbon dioxide (CO2) = 12.5 gmass of sulfur tetrafluoride (SF4) = 5.59 gMole fraction of…

Q: Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: The mole fractions are calculated using the following formulae. Mole fraction of N2=Number of N2…

Q: 4. A scuba diver carries a balloon containing 0.100 mole of a pure gas to a depth where the pressure…

A:

Q: Consider the following samples of gas: sample composition pressure temperature A 1.9 mol He (g) 1.8…

A: The Maxwell-Boltzmann distribution is a probability distribution that describes the distribution of…

Q: 1. A sample of neon gas occupies a volume of 9.60 L at 49.0°C and 0.620 atm. If it is desired to…

A: Since you have posted multiple non-related questions, we are entitled to answer the first 3 related…

Q: Kiki, Karl’s twin sister, did a lab just like our butane lab. But she did not have butane  as her…

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

Q: A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a…

A: The given data contains, CH4 =90.0%Ethane=8.9%Propane =1.1%Total Pressure =307.2 kPa

Q: 11. A mixture of 1.00 g of H2and 1.00g of He is placed in a 1.00L container at 27C. Calculate the…

A: PV=nRT P=nRT/V R=GAS CONSTANT(0.0821 L.atm/mol.K) Ptotal=p1+p 2+p 3...

Q: partial pressure of each gas in the mixture and the total pressure of the gas mixture.

A: Given mass of argon(Ar)=10g mass of Co2= 14.2g mass of Kr= 32.1 volume of gaseous mixture= 24.5L…

Q: 1. What mass of helium gas exerts a pressure of 1.20 atm in a volume of 5.40 L at a temperature of…

A: The partial pressure of each gas has same value which is 0.30377 atm this is because both are equi…

Q: partial pressure of each component of this gas

A: The total gas contains 90.0% of CH4, 8.9 % of C2H6 and 1.1% C3H8 So, Partial pressure of CH4 is –

Q: A 6.00 L tank at 16.8 °C is filled with 2.62 g of carbon dioxide gas and 5.02 g of sulfur…

A: Mass of Carbon dioxide (CO2) = 2.62 gMass of sulfur tetrafluoride (SF4) = 5.02 gMole fraction of…

Q: 10 moles of CH4, 20 moles of C2H6 and 70 moles of C3H8 are kept in a container. The mole fraction of…

A: Given that,  Moles of CH4 in container n1 = 10 mol Moles of C2H6 in container n2 = 20 mol Moles of…

Q: 11. A tank contains 5.00 moles of oxygen, 3.00 moles of neon, 6.00 moles of hydrogen sulfide, and…

A: Mole fraction is defined as the ratio of number of moles of the substance to the total number of…

Q: 11.) A mixture of neon and krypton gases contains neon at a partial pressure of 312 mm Hg and…

A: Mole fraction = total pressure/ partial pressure Total pressure = 312+446 = 758 mmHg

Q: A 10.0 L tank at 26.1 °C is filled with 12.8 g of dinitrogen difluoride gas and 3.26 g of dinitrogen…

A:

Q: The units for the ideal gas constant are Omol/L.k kPa.g OkPa.L komol O mol-L kPa.k O L.K mol-kPa…

A: In this question we have to find out the unit of the ideal gas constant.

Q: A mixture of carbon dioxide and helium gases at a total pressure of 798 mm Hg contains carbon…

A: In the Question-1 we want to determine the mass of the Helium in grams. You can see step by step…

Q: The partial pressure of CH4(g) is 0.175 atm and that of O2(g) is 0.250 atm in a mixture of the two…

A: a) Given that : Partial pressure of CH4 = 0.175 atm Partial pressure of O2 = 0.250 atm   Total…

Q: 11. A sample of gas isolated from unrefined petroleum contains 90.0% CH₁, 8.9% C₂H, and 1.1% C,H, at…

A: Partial pressure of a gas =  Mole fraction × Total pressure

Q: A mixture of 1.51 g H2 (Molar mass: 2.016 g/mol) and 17.73 g Cl2 (Molar mass: 71 g/mol) in a…

A: Given  mass of H2       = 1.51 gram  mass of Cl2      = 17.73 gram  Total Pressure  = 2.4 atm…

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.