Use the van der Waals equation of state to calculate the pressure of 2.60 mol of Cl2 at 469 K in a 5.60 L vessel. Use this list of van der Waals constants. CH4 2.303 2.273  0.0431  CO2 3.658 3.610  0.0429  Cl2 6.343 6.260  0.0542  NH3 4.225 4.170  0.0371  H2O 5.537 5.465  0.0305  Xe 4.192 4.137  0.0516 I've tried a few different ways and I'm still getting it wrong.

Q: A gas in a piston chamber kept in a constant-temperature bath at 28.22°C expands from 24.21 mL to…

A: For Vander wall gas, P =[{nRT/(V-nb)}- {an2 /V2}] (dS/dT)V= CV/ T, (dS/dV)T= (dP/dT)V = nR/(V-nb) S=…

Q: A sample of carbon dioxide is contained in a 500.0500.0 mL flask at 0.9760.976 atm and 15.615.6 ∘∘C.…

A: Given, Volume of the flask = 500.0 ml = 0.5 L pressure = 0.976 atm Temperature = 15.6 C° = (15.6 +…

Q: A 4.5-liter sample of gas at 760.0 T and 0.0°C is heated to 65°C. What volume must the gas occupy if…

A: Initial Volume, V1=4.5 L Initial temperature, T1=0.0°C + 273 =273 K Final temperatue=65°C =65 + 273…

Q: A sample of gas CH4 is observed to effuse through a pourous barrier in 7.53 minutes. Under the same…

A: The formula which relates time to effuse for a gas and molecular mass is shown below: Time for gas…

Q: A sealed container holding 0.0255 L0.0255 L of an ideal gas at 0.979 atm0.979 atm and 67 ∘C67 ∘C is…

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Q: 15.0 moles of gas are in a 8.00 L tank at 23.5∘C . Calculate the difference in pressure between…

A: Calculating the Pideal gas:

Q: A sealed container holding 0.0255 L0.0255 L of an ideal gas at 0.987 atm0.987 atm and 69 ∘C69⁢ ∘C is…

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Q: A 2.25 g sample of an unknown gas at 29⁢ ∘C and 1.00 atm is stored in a 1.45 L flask. What is the…

A: The given numerical can be solved as follows:

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: You have a 3.00-liter container filled with N, at 25°C and 1.75 atm pressure connected to a…

A: Given Gas Temperature  Pressure  Volume  Nitrogen (N2) 25oC = (25+273.15) =298.15 K 1.75 atm.…

Q: Use the van der Waals equation of state to calculate the pressure of 3.90 mol of Kr at 467 K in a…

A: The gas that possesses no particle interaction and whose particle’s collision is elastic is taken as…

Q: An unknown gas at 67.1 ∘C and 1.05 atm has a molar mass of 28.01 g/mol. Assuming ideal behavior,…

A: We will is use ideal gas equation to get the density.

Q: Convert 446,000 pascal, pa into torr

A: Given :- pressure = 446,000 Pa   To convert :- 446,000 Pa to torr  1 atm = 760 torr = 760 mmHg =…

Q: How can comparing the rates of effusion of gases X and Y allow the molar mass of Y to be calculated?…

A: Grahams’s Law of effusion states that the rate of effusion of a gas is inversely proportional to…

Q: E. 0.54 moles of helium and 0.32 moles are neon are combined in a 7.0 liter container at 25°C. What…

A: For question (E), we have to calculate the pressure exerted by a mixture of 0.54 moles of helium and…

Q: 4 447.9 780.7 115.5 71700 703 669 5 cm3 10 cm3 20 cm³ 09.1 726.0 411.1 796 822 20 cm3 10 cm3 5 cm3…

A: Boyle's law confirm this experiment .  At constant temperature the pressure of gas is inversely…

Q: A sample of an ideal gas has a volume of 2.33 L2.33 L at 282 K282 K and 1.09 atm.1.09 atm. Calculate…

A: The combination of various gas laws (Boyle, Charles as well as Gay Lussac) gives a generalized…

Q: According to the ideal gas law, a 10.06 mol sample of oxygen gas in a 0.8434 L container at 500.5 K…

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

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: STP (standard temperature and pressure) is used as a reference point for the molar volume of an…

A:

Q: A mixture of 30.74 moles of argon, 13.1 moles helium, 20.59 moles neon, and 42.99 moles krypton is…

A: Given data  T = 141.83 °C V= 2792.92 L  Number of moles are given of different gases

Q: A gas sample originally occupies 436mL at 24°C. When the volume is expanded to 612mL and the…

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Q: Based on their respective van der Waals constants, which of these two gases: Xe (a = 4.137 L2 atm…

A:

Q: A 0.530 mol sample of carbon dioxide gas occupies a volume of L at STP.

A: STP refers to standard temperature and pressure conditions. At STP, the standard temperature is 0oC…

Q: 15.0 moles of gas are in a 8.00 L tank at 23.4 ∘C . Calculate the difference in pressure between…

A: We have been given 15 moles of gas in an 8L tank  at 23.4 deg C.We have to calculate the difference…

Q: A 0.530 mol sample of neon gas occupies a volume of _______ L at STP.

A: • The values provided in the question are:-     i) Number of moles of Neon (Ne) gas sample = 0.530…

Q: The reaction for the combustion of naphthalene, C10H8, is C10H8 (s) + 12 O2 (g) → 10 CO2 (g) + 4 H2O…

A: The given reaction is as follows:   The volume carbon dioxide formed = 1.45 LThe pressure of carbon…

Q: Use the van der Waals equation of state to calculate the pressure of 3.00 mol of HI at 459 K in a…

A: Answer:The van der Waals equation of state for real gases is given by,

Q: A 1.62-mol sample of methane gas is maintained in a 0.660-L container at 305K. Calculate the…

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Q: Three glass bulbs, joined by closed stopcocks, have the following volumes and initial pressures of…

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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: A sample of neon gas effuses through a pinhole at a rate of 0.49 mL/s. What will be the rate of…

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Q: You have a 3.00-liter container filled with N₂ at 25°C and 1.75 atm pressure connected to a…

A: density of gas = total mass of gas / total volume Since mass = moles X molecular mass molar mass of…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Given data :

Q: Consider a reaction vessel of fixed volume containing 24.78 grams of nitrogen gas and 12.388 grams…

A: Answer: Final Pressure = 0.755 atm and Final volume = 40.3 L

Q: 2. Calculate the volume expected for 10.0 moles of acetylene gas at 15.0 °C and 200. atm, using…

A:

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A:

Q: What mass of Al₂O3 is produced when 13.2 L of O₂ gas react with Al at 434 K and 5.08 atm. 4 Al(s) +…

A: Given reaction is  4 Al(s) + 3O2 (g) →2Al2O3 (g) Temperature= 434 K Pressure = 5.08 atm Volume =13.2…

Q: How can comparing the rates of effusion of gases X and Y allow the molar mass of Y to be calculated?…

A: Grahm's Law of effusion of gases: This law is taken into consideration when two gases are compared…

Q: There are interactions between gas particles in an ideal gas. True

A: Given : an ideal gas  Tip : kinetic theory of gases tells that no interaction force between ideal…

Q: You have a perfect gas that undergoes thermal compression (constant temperature) which reduces its…

A: At constant Temperature: P1V1 = P2V2 P1 = initial pressureV1 = initial volumeP2 = final pressureV2 =…

Q: Use the van der Waals equation of state to calculate the pressure of 3.20 mol of CH, at 479 K in a…

A: Given that, for CH4  The number of moles is n = 3.20 mol, The temperature is T = 479 K, The volume…

Q: Effusion is the process where a gas flows through a small hole in a container.  Graham’s Law of…

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Q: A flask contains a mixture of two gases: NO2 and Ne. The flask holds 0.519 mol of NO2 and an unknown…

A:

Q: An unknown gas at 73.1 ∘C and 1.05 atm has a molar mass of 44.10 g/mol. Assuming ideal behavior,…

A: Ideal gas equation is the equation which obeys all gas laws under all condition of temperature and…

Q: C,HBO7(s) +3 NaHCO3(s) + H2O(1) --> NagCgHgO7(s) + 3H2O(I) + 3CO2(g) 228.2 g C6H807(s) is reacted at…

A: Given Temperature = 265 K Volume = 158 L Mass of C6H8O7 = 228.2 g Molar Mass of C6H8O7 = 192.1 g/mol