Exactly equal amounts (in moles) of gas A and gas B arecombined in a 1-L container at room temperature. Gas B has amolar mass that is twice that of gas A. Which statement is truefor the mixture of gases and why?a. The molecules of gas B have greater kinetic energy than thoseof gas A.b. Gas B has a greater partial pressure than gas A.c. The molecules of gas B have a greater average velocity thanthose of gas A.d. Gas B makes a greater contribution to the average density ofthe mixture than gas A.

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

A: Ideal gas equation:Since, there is no leakage of the gas, therefore number of moles n will be…

Q: Collisions between gas particles or with the walls of the container are elastic, meaning no energy…

A: The kinetic theory of gases explains the macroscopic properties of gases, such as volume, pressure,…

Q: A sample of Cl₂ gas has a volume of 17.0 L at a pressure of 1.50 atm and a temperature of 23 °C.…

A:

Q: A sample of helium gas collected at a pressure of 1.11 atm and a temperature of 10.0°C is found to…

A: According to ideal gas law, PV = nRT where P = pressure in atm = 1.11 atm  V = volume in L = 23.9 L…

Q: How can the pressure of a mixture of gases be described? O a standard pressure ratio between partial…

A: Pressure of gases in mixture can be explained on the basis of a law .

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

A:

Q: Expansion of a gas with no change in number of moles of gas at constant temperature results in an…

A: Answer:- This question is answered by using the simple concept of gaseous laws which states that the…

Q: A quantity of hydrogen gas occupies a volume of 30.0 mL at a certain temperature and pressure. What…

A: To solve this problem, use the Combined Gas Law equation. The combined gas law is a fundamental…

Q: 4. A nitrogen gas with a volume of 11.75 L was placed inside a chamber with a pressure of 2022 psi…

A:

Q: A sample of gas at 29.8ºC has a volume of 6.4 L and exerts a pressure of 762 mm Hg. How many moles…

A:

Q: 1. At STP, gases have a volume of 22.4 L per mole. RTP is room temperature (25 °C) and pressure (1…

A: Given: Number of moles of gas = 1 mol. Temperature = 25°C                         = (25+273)K = 298…

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

A: Information about the question

Q: wo identical pressurized-gas cylinders contain two different gases: N2 and H2 The cylinders have…

A: Given that the cylinders contain two different gases N2 and H2 of equal masses and at the same…

Q: Ideal Gas Law A gas that contains 4.01mol of gas at 5.66atm and takes up 12.1L. what is the…

A:

Q: the pressure on a 2.66L volume of gas is 1.14atm and we decrease the volume of the container to…

A: We will use Boyle's law

Q: A sample of xenon gas that occupies a volume of 43.4 L at a temperature of 0 °C and a pressure of 1…

A:

Q: .What is the temperature of gas, in K, that is expanded from 2.5 L at 25 C to 4.0 L at constant…

A:

Q: If N, is added to a balloon that contains O, (partial pressure 400 mm Hg) and CO, (partial pressure…

A: 1- We will calculate the partial pressure of each gases after addition of N2 gas in a balloon that…

Q: A sample of neon gas at a pressure of 774 mm Hg and a temperature of 44 °C, occupies a volume of…

A: Here given--- Initial Pressure (P1) = 774 mmHg = (774/760) atm = 1.018 atm Initial Volume (V1) =…

Q: A sample of gas at 33.9ºC has a volume of 10.3 L and exerts a pressure of 782 mm Hg. How many moles…

A: To solve this problem, we need the universal gas equation which is given as follows: PV=nRT Here, P…

Q: A sample of krypton gas that occupies a volume of 12.7 L at a temperature of 0 °C and a pressure of…

A: Ideal gas equation is  PV = nRT  P = pressure of the gas  V = volume  n = moles of the gas  R = gas…

Q: 5. A 27.0 mL sample of neon gas at 475 mmHg is cooled from 110°C to 30°C. If the volume remains…

A: Ideal gas equation PV =  nRT used.

Q: A sample of hydrogen gas at a pressure of 817 mm Hg and a temperature of 47 °C, occupies a volume of…

A: Given :  pressure is constant (817 mm Hg) Initial temperature = 47°C  Initial volume = 7.96 L  Final…

Q: .  If 10.0 L of neon gas exerts a pressure of 25.0 atm at 50oC, how many moles of neon are present

A: For ideal gas we know that PV = n RT  Where, at pressure P and temperature T  ,volume  of n mol of a…

Q: A sample of carbon dioxide gas at a pressure of 0.556 atm and a temperature of 21.2°C occupies a…

A:

Q: 2.0 moles of  Ne gas are placed in a steel box and the pressure is measured. An identical box at the…

A: Answer :option b is the correct answer The pressure in the both box will be equal . We know  PV=nRT…

Q: The volume of one mole of nitrogen gas at STP is 22.4 L.  The density of liquid nitrogen at -196oC…

A: Here we use the formula                       Density = mass/volume

Q: mol of gas. A 2.80 L flask filled with gas at 0.914 atm and 19.0 °C contains

A: Convert unit of temperature:

Q: A sample of gas in a cylinder has an initial volume of 40.0L and it has 1.7 moles of gas. The next…

A: Avogadro’s law, is a gas law which states that the total number of atoms/molecules of a gas (i.e.…

Q: A gas originally at 25oC and 1.50 atm pressure in a 2.3 liter container is allowed to expand until…

A:

Q: moles of gas. A sample of oxygen gas that occupies a volume of 15.0 L at a temperature of 0 °C and a…

A: Given, Volume of oxygen gas, V = 15L Temperature , T = 0° C = 273.15K Pressure, P = 1 atm

Q: Не %3D = N2 (i) (ii) (ii) Consider the samples of gases pictured above. If the three samples are all…

A: Standard data: The molar mass of He = 4 g/mol The molar mass of N2 = 28 g/mol

Q: 1.What volume would be occupied by 0.50 moles of a gas at a temperature of 35ºC and at a 1 atm of…

A:

Q: f 0.211 g of a gas occupies 204.5 mL at STP, what is the molecular weight of this gas? R = 0.08206…

A: First, we need to convert the volume of the gas from milliliters to liters because the gas constant…

Q: moles of gas. A sample of oxygen gas that occupies a volume of 36.2 L at a temperature of 0 °C and a…

A:

Q: 35. Calculate the mass of nitrogen dioxide gas occupying a vol- ume of 2.50 L at 35 °C and 0.974 atm…

A: Given that: Volume of NO2 = 2.50 L T = 35°C = 35°C+273 = 308 K P = 0.974 atm

Q: A sample of Hydrogen gas collected at a pressure of 1.28 atm and temperature 12 C. Is found to…

A: According to Ideal Gas law PV = nRT n =  Where P = pressure of system V = volume if system n = moles…

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.