Use the van der Waals equation of state to calculate the pressure P of 3.50 mol of Cl2 at 493 K in a 4.00 L vessel. Use this list of van der Waals constants. P=_________atm  Use the ideal gas equation to calculate the pressure P under the same conditions. P=__________atm

Q: Use the References to access important values if needed for this question. STP (standard temperature…

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Q: A mixture of cyclopropane gas, C3H6, and oxygen, O2, in a 1.00:4.00 mole ratio is used as an…

A: Answer :- 84800 Pa  The partial pressure of O2 = 84800 Pa.…

Q: For oxygen gas, the van der Waals equation of state achieves its best fit for a = 0.14 N.m²/mol² and…

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Q: The volume of a gas that fits the van der Waals equation at a given temperature and pressure of 4.00…

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Q: 8.8 For a mixture of 0.0786 mol of C,H, and 0.1214 mol of CO, in a 700.0-cm container at 40°C,…

A: Given: moles of C2H4 = 0.0786 mol moles of CO2 = 0.1214 mol Volume of container = 700.0 cm3 = 0.7 L…

Q: Calculate the pressure exerted by 0.5100 mole of N2 in a 1.0000-L container at 25.0°C. (The gas…

A: Given : Moles of gas N2 = 0.5100 mol. Volume of container = 1.0000 L And temperature = 25.0 oC

Q: to form Cl2 and NaF. Use the ideal gas law equation to determine the mass of NaCl that reacted with…

A: Given :  Volume = 15.0 L Pressure = 1.50 atm  Temperature = 280 K R = 0.082 L.atm/mol.K Moles = ?…

Q: A particular mass of N2 occupies a volume of 1.00 L at –50 °C and 800 bar. Determine the volume…

A: Answer: Ideal gas law: PV=nRTPVT=nRhere:P=pressure of the gasV=volume occupied by the gasn=number of…

Q: . A certain gas obeys the van der Waals equation with a = 0.50 m6 Pa mol-2. Its volume is found to…

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Q: The van der Waals equation of state for a real gas is n?a P+ v2 - nb]= At what pressure will 1.00…

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Q: A 2.00 liter evacuated container has a mass of 1050.0g. When the container is filled with an unknown…

A: Given : Mass of conatiner without gas = 1050.0 g Mass of conatiner with gas = 1052.4 g Volume(V) =…

Q: A 10.00 L tank at 21.4 °C is filled with 14.8 g of carbon monoxide gas and 10.7 g of sulfur…

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Q: p+a |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles…

A: Given :

Q: According to the ideal gas law, a 0.9244 mol sample of oxygen gas in a 1.983 L container at 268.1 K…

A: As per Bartleyby guidelines i answered only first question so please don't mind. Kindly post other…

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: Use the References to access important values if needed for this question. According to the ideal…

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Q: Use the van der Waals equation of state to calculate the pressure of 3.50 mol of H, S at 493K in a…

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Q: The van der Waals equation of state for a real gas is n²a P+ y2 nb| = nRT At what pressure will 1.00…

A: Given, Temperature(T) =  298 K moles(n) = 1 mol volume(V) = 10 L a = 2.253 atm L2 /mol2 b = 0.04278…

Q: Calculate the pressure exerted by 1.0 mol of hydrogen at 0°C in a vessel with volume of 5.0 dm3…

A: a) Given that : Mol of hydrogen (n) = 1.0 mol Temperature (T) = 0°C = 273 K Volume (V) = 5.0 dm3 =…

Q: CH4 storage tank with a volume of 49.0 L. When empty, the tank has a mass of 55.85 kg, and when…

A: Given that,  Volume of tank V  = 49.0L Mass of CH4 filled in tank m  = 62.07 - 55.85…

Q: According to the ldeal gas law, a 0.9434 mol sample of oxygen gas in a 1.900 L container at 272.0 K…

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Q: Carbon monoxide and molecular oxygen react to form carbon dioxide. A 50.0 L reactor at 25.0 oC is…

A: Initial Pressure of Co = 1 bar total pressure = 3.59 bar, so initial pressure of O2 = 3.59-1=2.59…

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

A: Given: At STP  Temperature, T = 0°C, Pressure, P=1 atm Molar volume= 22.4 L /mol

Q: 3.5 moles of NH; occupy 5.20 L at 47°C. Calculate the pressure of the gas in atm using: a)The ideal…

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Q: Use the van der Waals equation of state to calculate the pressure P of 2.40 mol of CH, at 499 K in a…

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Q: The pressure and temp of 1L of a gas are increased from 0°c and 1 atm to 100°c and 1520 mmg . so the…

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Q: Using (a) the ideal gas law and (b) the van der Waals equation, calculate the pressure exerted by…

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Q: 1. In a 100mL sealed flask, 0.1 g of H2 gas reacts with 0.15 g of N2 gas to generate NH3 gas at 25…

A: The reaction between H2 and N2 is written as, N2(g) + H2(g) → NH3(g) Multiply NH3(g) with 2 and…

Q: Use the van der Waals equation of state to calculate the pressure of 2.70 mol of HCl at 495 K in a…

A: Given: HCl gas: n = 2.70 mol Temperature = 495K Volume= 4L Vander Waal constants, a=3.648atmL2mol-2…

Q: The experimental Boyle temperature / K 110 327 Gas The a constant of the van der Waals equation /…

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Q: 11. A rigid 8.80 L container is charged with 0.700 mol of helium gas at 9.00 C. An identical…

A: Given :   Volume of both container = 8.80 L  Moles of He gas = 0.700  Moles of CO2 gas = 0.700…

Q: (a) A 4.25-L flask contains 3.46 mol CO2 at 229 °C. The pressure of this gas calculated from the…

A: Hg

Q: According to the ideal gas law, a 1.042 mol sample of methane gas in a 1.670 L container at 267.2 K…

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Q: Calculate pressure using the idéal gás láw and the vấn der Wäals equation. A 1.79-mol sample of…

A: Given : Moles of oxygen gas = 1.79 mol  Volume of container = 0.754 L And temperature = 308 K

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

A: Given the molar volume at STP = 22.4 L/mol Required conversion factor is: 1 mol = 22.4 L

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…

Q: The compound BF3 has van der Waals constants a = 3.980 atm•L2 /mol2 and b = 0.0544 L/mol. Using both…

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Q: Calculate the pressure exerted by 0.5900 mole of  in a 1.1000-L container at 25.0°C. (The gas…

A: 1.

Q: Use the van der Waals equation of state to calculate the pressure of 2.30 mol of HF at 451 K in a…

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Q: Use the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of…

A: Given that Number of moles of Neon, n = 1.000 mol Pressure of Neon, P = 500.0 atm Temperature of…

Q: A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the…

A: Given,Volume (V) = 1.00 LNumber of moles (n) = 1 molTemperature (T) = 25 oC = 298 K

Q: Use the van der Waals equation of state to calculate the pressure of 3.20 mol of HBr at 459 K in a…

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Q: The pressure exerted by 4 mole of CO2 at 90°C when it occupies 1 Liters knowing that: a = 3.61 1atm…

A: According to the Van der Waals Equation the pressure of the gas can be calculated as follows:…

Q: Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a…

A: We have to calculate the pressure by using van der Waals  equation of state as follows in step 2:

Q: O VPN O 80% b) What does this equation correct for that the Ideal Gas does not? Van der Waals ea…

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Q: Using the van der Waals equation, calculate the temperature of 20.0 mole of helium in a nRT n?a 10.0…

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Q: Pressure and temperature affect the amount of space between gas molecules, which affects the volume…

A: Part A An ideal gas is an imaginary gas that does not have any force of interaction, does not lose…

Q: use the vander waats equation of state to calculate the pressure p of 3.40 mol of 1₂0 at 475k in a…

A: The ideal gas equation is PV = nRT It is a formula used for determining a gas's pressure, volume,…

Q: 2 p+a- |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for…

A: The van der Waals gas equation is given by, where where P = pressure V = volume n = moles R = gas…

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.