The van der Waals equation of state for a real gas is n²a' = nRT At what pressure will 1.00 mole of NH3 be in a 10.00 L container at 298 K assuming NH3 is a real gas. (van der Waals constants for NH3 are a = 4.170 L² atm mol2, b=0.03707 L mol-4) O 2.03 atm O 2.41 atm O 20.3 atm O 24.1 atm O 2.47 atm

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

A: We are given two gases Xe and CO2 along with their respective Van der Waals constant values.

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…

A:

Q: What is the pressure in atm of a gas where n = 0.88 mol, V = 5.19 L, and T = 15.6oC?

A: Here for a gas, mole number, volume and temperature are given, we need to calculate the pressure of…

Q: A 5.31 mol sample of O2(g) is placed in a 1.00 L flask at 100.0°C. What is the pressure (in atm) of…

A:

Q: mixture contains 10.0 g N2 amd 10.0 g of CO2 in a 2.55 L container at 25 degrees C.    - Calculate…

A:

Q: The unbalanced equation for combustion of ethane is: C₂H6(g) + 0₂(g) →→→ CO₂(g) + ______ H₂O(g).…

A: The objective of the question is to give-Balanced Equation.The final pressure.

Q: A mixture made up of 2.0 moles of N2 and 3.0 moles of H2 (g) exerts total P= 4.0atm. Calculate the…

A:

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: A combustion reaction involving 628.0 g n-butanol (C,H100) occurs at 345.0 °C and 15.2 atm. What…

A: Given :-  Amount of butanol = 628.0 g  Temperature = 345.0 °C  Pressure = 15.2 atm  To calculate :-…

Q: What is the mole fraction of the N2 in the system? 10.00g of O2 and 15.00g N2 are combined in a…

A: Mass of O2 = 10.00 g  Mass of N2 = 15.00 g Molar mass of N2 = 28.02 g/mol Molar mass of O2 = 32.00…

Q: What is the density (in g/Lg/L) of hydrogen gas at 24 ∘C∘C and a pressure of 1670 psipsi?…

A: Density (d) =massvolume = mV

Q: The van der Waals equation compensates for non-ideal behavior of gases by taking into account…

A: Given: The moles of CO, (n) = 1.5 moles. The volume of the flask, (V) = 3 L. The temperature, (T) =…

Q: Part 1. A chemist reacted 12.0 liters of F2 gas with NaCl in the laboratory to form Cl2 gas and NaF.…

A: Given: Volume (V), F2 used = 12 L The pressure (P) = 1.5 atm Temperature (T) = 28 K Standard P, T…

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

A: The van der-Waal's equation is given by (P+an2V2)(V-nb)=nRT R = gas constant n = number of moles of…

Q: You start with an equimolar mixture of the gases SO₂ and O₂ in a container. The SO₂ and O₂ react to…

A: Ideal gas equation is given by PV=nRT where P is the pressure, V is the volume, n is the number of…

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

A: Given :  Assume nitrogen (N2) as an ideal gas at temperatures above its boiling point of -196 °C T1…

Q: An unknown gas at 77.1∘C  and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior,…

A: The formula required to determine the density of gas with ideal behavior is as follows,

Q: of total mass 80g. 14% of the total mass is nitrogen. The nitrogen is occupying a volume of 0.995…

A:

Q: A flask contains a mixture of two gases: NO2 and Ne. The flask holds 0.788 mol of NO2 and an unknown…

A:

Q: ired to decrease the volume of the gas sample to 7.44 L, p 0.540 atm, the temperature of the gas…

A: Initial Volume = 9.40 L Initial Temperature =53 °c = 326 K Initial pressure = 0.440 atm Final…

Q: According to the ideal gas law, a 1.039 mol sample of nitrogen gas in a 1.269 L container at 266.5 K…

A: Answer:Given data:

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

A:

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

A:

Q: temperature T for gases better than the Ideal Gas Law does: p+₁²/²2 (₁ (V-nb)=nRT The parameters a…

A:

Q: According to the ideal gas law, a 1.001 mol sample of krypton gas in a 1.235 L container at 269.9 K…

A: Given : Moles of gas = 1.001 mol. Volume = 1.235 L Temperature = 269.9 K a = 2.318 L2.atm/mol2  b =…

Q: Using Ideal Gas Law    25.0g of methane (CH4) has a pressure of 450.0kPa at 250℃. Find the volume…

A: Ideal gas law  states that the product of pressure and volume of one gram molecule is equal to the…

Q: Consider the following reaction: 2H2O(l) -> 2H2(g) + O2(g)…

A:

Q: A sample of neon gas is held in a rigid 6.351L container with a pressure of 1.026 atm at 22.9°C.…

A: Answer:Here:

Q: A gaseous compound containing 62.45% chlorine and 37.55% nitrogen by mass are held at standard…

A:

Q: If 2.1 moles of aluminum react with 2.3 moles of chlorine gas, how many moles of AICI3 may form?…

A: Consider the balanced equation for the reaction of aluminum and chlorine gas is as follows; 2 Al…

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

A:

Q: As part of the rock analysis, a student added hydrochloric acid to a rock sample and observed a…

A:

Q: A 4.17 g4.17 g sample of NH3NH3 gas and a 4.17 g4.17 g sample of HClHCl gas are mixed in a 2.00…

A: GIVEN: NH3 gas sample =  4.17 g HCl gas sample = 4.17g Volume of flask =2.00 L Temperature=25oC To…

Q: What is the pressure of a 50.0 L tank that contains 4.04 kg of oxygen, O2, at 24 degrees C? Assume…

A: According to ideal gas equation,

Q: Use the van der Waals equation of state to calculate the pressure of 4.00 mol of SO, at 453K in a…

A: Since you have posted multiple questions according to guidelines I am solving first one,if you want…

Q: What assumption (s) are used in kinetic molecular theory to define an ideal gas?

A: Assumption (s) are used in kinetic molecular theory to define an ideal gas are,   The energy and…

Q: Suppose the Ideal Gas Law is p=(nRT^2)/(V^2). Evaluate these derivatives: a. ((∂p/∂T))n,V b.…

A: Ideal gas law is a relation between pressure, volume and temperature of a gas.

Q: What is the volume for a gas where Y=260 K, P=2 atm, n=0.05 mol?

A: Given:  Temperature, T = 260 K  Pressure, P = 2 atm  Number of moles = n = 0.05 moles

Q: at what temperature will the molar volume of chlorine gas at 2.38 atm be 12.3 L/mol. Assuming the…

A: Solution -

Q: Consider two hypothetical gases, gas A and gas B, which have the following Van der Waals constants:…

A: The pressure of Gas B will deviate less than the pressure of Gas A from the pressure predicted by…

Q: If 16.5 mol16.5 mol of an ideal gas is at 5.19 atm5.19 atm at 97.40 ∘C,97.40⁢ ∘C, what is the volume…

A: The ideal gas equation is given by,                                            PV = nRT Where, P is…

Q: Entonox is an anaesthetic gas containing 50% oxygen and 50% nitrous oxide(N2O). If 200L of the gas…

A: Data

Q: Using the ideal gas law (PV=nRT), calculate how many moles of air are in the lungs of an average…

A: Using ideal gas law we can write pV = nRT Where p = Pressure of system  V = volume of gas n = moles…

Q: 5. After blowing up a balloon, a student was curious what the partial pressure of each gas was in…

A: Daltons Law of partial pressure says that total pressure is the sum of the individual pressures of…

Q: Which of the graphs below shows the relationship between the molar volume and molar mass of ideal…

A: Avogadro rule: According to this rule, if the temperature and pressure of the gases are the same…

Q: Water vapor is a polar gas molecule. Because of this it has fairly strong interactions with itself…

A:

Q: When 4.4 grams of NH4NO3 is decomposed in a closed container, it will produce N2, O2 and water vapor…

A: The partial pressure of nitrogen gas is calculated in step two.

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.