Use the van der Waals equation of state to calculate the pressure ? of 4.00 mol of CH4 at 469 K in a 4.20 L vessel

Q: P1A.8 A vessel of volume 22.4 dm' contains 2.0 mol H,(g) and 1.0 mol N,(g) at 273.15 K initially.…

A: Partial pressure:  It is the individual pressure of a gas when a mixture of gases is present in a…

Q: How many moles of chlorine at 110 degrees C at 28.0 atm would occupy a vessel of 15.0 L?

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Q: tractive forces between the particles), the larger the van der Waal constant a. The larger the…

A: Vanderwaal's constant "a" represents  for inter-molecular forces constant "b" is a correction for…

Q: What volume of carbon dioxide in liters could be generated at 0.995 atm and 445. K by the combustion…

A: Given is , P= 0.995 atm T=445 K Mass of C5H12= 244.20 g R= 0.08206 L.atm/mol.K V=? And we know,…

Q: Calculate the pressure (in atm) of a 2.90 mol sample of CO₂ gas at 475 K in a 0.750 L container…

A: Given: Number of moles (n) is 2.90 mol a is 3.59 L2atm/mol2 b is 0.0427 L/mol V is 0.750 L T is 475…

Q: A gas, behaving ideally, has a pressure P1 and at a volume V1. The pressure of the gas is changed to…

A:

Q: Calculate the pressure (in atm) of a 5.60 mol sample of neon gas at 500.0 K in a 1.00 L container…

A: The moles of sample neon gas = 5.60 mol The temperature of the gas = 500.0 KThe volume of the gas =…

Q: What volume does 0.118 mol of helium gas at a pressure of0.97 atm and a temperature of 305 K occupy?…

A: For He gas : Ideal gas equation : PV = nRT 0.97 x V = 0.118 x 0.0821 x 305  V = 3.046 L For Ar gas :…

Q: A sample of 1.00 moles of oxygen at 50℃ and 98.6 kPa occupies what volume?

A: According to ideal gas law, PV = nRT where P = pressure in atm = pressure in KPa / 101.325 = 98.6 /…

Q: suppose that 2.96 moles of heluim gas occupies a 73.3L tank what temp will the pressure in the tank…

A: Given, moles of helium gas = 2.96 mol            volume = 73.3 L            pressure = 550 mm Hg =…

Q: A balloon is filled with 2 liters of air at sea level. If the balloon is taken up a mountain so that…

A: Given: The standard pressure at the sea level, P1 = 1 atm The volume of the balloon, V1 = 2 L The…

Q: Use the van der Waals equation of state to calculate the pressure of 3.90 mol of N,0 at 453K in a…

A: Answer: This question is basically asking us to compare the pressure of the gases when they are…

Q: A sample of NH3 gas is observed to effuse through a pourous barrier in 3.61 minutes. Under the same…

A: According to Graham’s diffusion law, the rate of effusion of gases is inversely proportional to the…

Q: What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 45.0 g He at 25o…

A: Given mass of He = 45 g volume = 10 L Temperature = 25°C = 25+273 = 298°K

Q: Calculate the pressure (in atm) of a 5.70 mol sample of nitrogen gas at 200.0 K in a 2.00 L…

A: Number of moles (n) = 5.70 mol Temperature (t) = 200.0 k Volume (V ) = 2.00 L a = 1.39 L²･atm/mol² b…

Q: Calculate the pressure (in atm) of a 3.10 mol sample of ammonia gas at 350.0 K in a 3.00 L container…

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Q: How many moles of chlorine gas at 120 C and 33.3 atm would occupy a vessel of 36.5L?

A: The gaseous state is the state of matter with least intermolecular force of attraction between…

Q: 258 mL sample of MEK , an industrial solvent, is found to have a mass of 0.599 g at 0.988 atm and…

A:

Q: 0.291 g

A: Mg + 2HCl -----> MgCl2 + H2

Q: Calculate the molar mass of a gas at 458. torr and 99.0 °C if 206, ng occupies 0.206 μl.. Be sure…

A: The question is based on the concept of ideal gas equation.We need to calculate molecular mass of…

Q: What is the volume of 0.5 moles of SO2 gas at 150. kPA and 50.C

A: The Ideal gas equation is expressed as,

Q: According to Avogadro's Principle at STP 1.00mole of a gas will occupy 22.4L. What are the…

A: Ans

Q: calculate the pressure ?P of 3.90 mol3.90 mol of NH3NH3 at 453 K453 K in a 4.40 L4.40 L vessel. Use…

A: Answer : pressure (p)for ideal gas = ? Moles(n)= 3.9 Temperature (T)=453 K  Volume (V)=4.4L  Gas…

Q: Explain the pressure-moles relationship with kinetic molecular theory.

A: The pressure-moles relationship describes the behavior of gases in response to changes in pressure…

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: Calculate the pressure (in atm) of a 3.30 mol sample of ammonia gas at 350.0 K in a 3.00 L container…

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Q: In the Van Der Waals Equation for real gases what are the a and b variables and how to they adjust…

A: Vanderwall gas molecule have attraction between gas molecules  and they have significant size of…

Q: 3.19K HI B. What mass of aluminum metal must be dissolved in excess hydroiodic acid to pro L of…

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Q: Using the van der Waals equation of state, calculate the molar volume of 1 mole of a gas at a…

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Q: Use the van der Waals equation of state to calculate the pressure P of 3.60 mol of H,O at 479 K in a…

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Q: Use the van der Waals equation of state to calculate the pressure of 3.70 mol of SO, at 499K in a…

A: Given :  Moles of gas SO2 = n = 3.70 mol  Temperature = T = 499 K Volume of vessel = V = 3.50 L  We…

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.