A 5.00-L cylinder initially contains 0.200 mol Br2 and 2.00 mol F2 at 275 K.  Assuming 100% yield of BrF5 and constant temperature, calculate the final pressure (atm) of Br2.   Br2 (g)   +   F2 (g)     -->     BrF5 (g)

Q: A 1.50 L bulb containing He at 155 torr is connected by a valve to a 2.00 L bulb containing CH 4  at…

A: Given: Volume of bulb containing helium= 1.50L Pressure of He= 155 torr Volume of bulb containing…

Q: Calculate the density of Xenon gas (in g/L) at 23.0oC and 700.0 torr.

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

Q: For the given reaction, what volume of O, would be required to react with 8.8 L of SO,, measured at…

A: One mole of a substance contains 22.414 L by volume at STP. From a balanced reaction and reaction…

Q: You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask…

A: Number of moles of CO2 in the flask initially is calculated using Ideal Gas equation as follows,1…

Q: A sample of xenon gas occupies a volume of 6.95L at 431K. If the pressure remains constant, at what…

A: Initial volume, V1 = 6.95 L Initial temperature, T1 = 431 K Final volume, V2 = 3.77 L Final…

Q: Ammonia and hydrogen chloride gases react to form solid ammonium chloride. A 12L reaction flask…

A: This question is based on Ideal gas equation. Applying the concept of ideal gas equation you can…

Q: 60 L tank containing 2.5 mol of CH4 . Initially, when Poutside was 1 atm, there was no leakage. But…

A: Given: Volume of tank = 60 L Initial moles of CH4 = 2.5 mol. Initial pressure of CH4 = 1.0 atm. And…

Q: If a gaseous mixture is made by combining 4.77 g Ar and 2.34 g Kr in an evacuated 2.50 L container…

A: Pi = Xi x P Where, Pi = partial pressure of gas i,             Xi = mole fraction of gas i…

Q: A 10.18 mol sample of nitrogen gas is maintained in a 0.8418 L container at 303.3 K. What is the…

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Q: If a gaseous mixture is made by combining 3.07 g Ar and 2.59 g Kr in an evacuated 2.50 L container…

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Q: Consider separate 1.0 liter gaseous samples of N2, Ar, CH4, and CO2 all at STP. (a) Rank the gases…

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Q: The combustion of octane, C,H18, proceeds according to the reaction shown. 2 C3H18(1) + 25 0,(g) –…

A: The balance chemical reaction :  2C8H18(L) + 25O2(g) ----> 16CO2(g) + 18H2O(L)  Number of moles…

Q: A 5.73-L flask at 25 °C contains 0.0388 mol of N2, 0.147 mol of CO, and 0.0803 mol of H2. What is…

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

Q: A gas with a mass of 95.14g occupies 48.8L at 659mmHg and 25.3°C. What is its molecular weight? Use…

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Q: A 1.00-L gas sample at 100.°C and 650. torr contains 53.0% helium and 47.0% xenon by mass. What are…

A: Formula that we use: 1. pi=xptotal     where pi=partial pressure of the gas, x=mole fraction of that…

Q: In dry atmospheric air, the four most abundant components are N2, X = 0.808; O2, X = 0.1915; Ar, X =…

A: Given:Mole fraction of O2 (XO2)= 0.1915.Total atmospheric pressure (PTotal) = 1 atm = 760 torr.

Q: A gaseous mixture is made by combining 3.92 g Ar and 4.57 g Kr in an evacuated 2.50 L container at…

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Q: A 20.0L tank contains 0.225 kg of helium at 18 degrees celcius. The molar mass of helium is 4.00…

A: Given : Volume of tank = 20.0 L Mass of helium gas = 0.225 Kg = 225 g…

Q: Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of…

A: Given: 1) Temperature =340°C =(340+273)K 2) Pressure = 6.75 atm 3) Mass of sulfur = 5.70 g 4)…

Q: A large flask with a volume of 936 mL is evacuated and found to have a mass of 134.66 g. It is then…

A: step 1: Here, given as the: Thus, the mass of gas is 1.38g. Now, to calculate the molar mass,…

Q: Calculate the density of Freon 12, CF2Cl2, at 30.0 °C and 0.954 atm.

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

Q: In dry atmospheric air, the four most abundant components are N2, X = 0.808; O2, X = 0.1915; Ar, X =…

A: Air is a gaseous mixture of different gases. These gases are present in different mole fractions in…

Q: A sealed flask contains 3.1 L of a gas at 2.4 atm and 22.7 °C. If the density of the gas is 9.7 g/L,…

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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: You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask…

A: The total mass of the mixture = 6.35g Consider the mass of BaO and MgO in the unknown sample be 'x'…

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

A:

Q: A large flask with a volume of 936 mL is evacuated and found to have a mass of 134.66 g. It is then…

A:

Q: You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask…

A: Convert the given temperature that is 30 degree Celsius in kelvin as shown follows:T (K) = (30 +…

Q: A 3.00-L gas sample at 100. ̊C and 600. torr contains55.0% helium and 45.0% xenon by mass. What are…

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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: 1.00 mole of O2 and 2.00 moles of NH3 are placed in a container and allowed to react at 850…

A: 1.00 mole of O2 and 2.00 moles of NH3                                       4 NH3(g)    +   5 O2(g)…

Q: (1) The following gases were mixed and placed in a 10-L container at STP: 1.00g He, 0.50g Xe, and…

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Q: Three 1.00 L flasks at 25.0 °C and 1013 kPa pressure contain: CH4 (flask A), CO2 (flask B) and NH3…

A: The volume, temperature and pressure of three flasks (flask A, flask B and flask C) is 1.00 L,…

Q: ulfur burns in oxygen with a deep blue flame to produce sulfur dioxide.  If 5.85 g S8 and 1.00 atm…

A: Given : Mass of  S8 = 5.85 g  Pressure of 02 = 1 atm Volume = 5.00 L

Q: What is the partial pressure of He in a 5.00-L vessel at 25ºC that contains 0.0410 mole of He, 0.121…

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Q: 4 NH3 (g) + 5 O2 (g) = 4 NO (g) + 6 H2O (g)A sample of NH3 is added to an initially evacuated 2.00 L…

A: Given dataPartial pressure of NH3= 415torrPartial pressure of O2 = (875-415) torr…

Q: 238.15L of gas at 841.5 torr and 85.1°C is heated until the temperature reaches 134.1°C.  and the…

A: According to the ideal gas law, the volume of a gas is directly proportional to the number of moles…

Q: A 4.00-g sample of a mixture of CaO and BaO is placed in a1.00-L vessel containing CO2 gas at a…

A: First we have to calculate the reacted pressure of CO2 gas in the given reaction:- The initial…

Q: Based on their respective van der Waals constants, which of these two gases: or Ar (a = 1.337 L² atm…

A: On the basis of Van der waals constant  we can easily  judge  and compare the ideal gas behavior…

Q: 1.734×10-4 mol of an unidentified gaseous substance effuses through a tiny hole in 93.2 s. A) Under…

A: According to Graham's law of effusion, the rate of effusion of a gas is inversely proportional to…

Q: You placed 6.35 g of a mixture containing unknown amounts of BaO(s) and MgO(s) in a 3.50-L flask…

A: From given datas  With ideal gas equation we are calculating initial and final number of moles of…

Q: A 3.75 L sample of gas from a chemical plant is collected and analyzed st 25 degrees celisus. It is…

A: The number of moles for a given chemical species refers to the ratio of mass of the species to that…

Q: The combustion of octane, C8H18 proceeds according to the reaction shown.…

A:

Q: Based on their respective van der Waals constants, which of these two gases: Ar (a = 1.337 L2 atm…

A:

Q: The combustion of octane, C,H,8, proceeds according to the reaction shown. 2C,H,;(1) + 25 0, (g) →…

A:

Q: A sample of H, with a pressure of 1.89 atm and a volume of 274 mL is allowed to react with excess N2…

A: The combination of Boyle's law, Charles's law and Avogadro's law leads to an equation which gives…

Q: A 2.00 L container holds 4.00 moles of O2 and 2.70 moles of He at 293K. What is the partial pressure…

A: Dalton's Law of partial pressures :-  The toatal pressure of a mixture of non reacting gases is…

Q: 9) A 0.780 L flask is filled with 2.88 mol of acetylene gas (C2H2). Given that the pressureexerted…

A: GivenVolume of the gas = 0.780LMoles of gas= 2.88Pressure of the gas = 3.60 atmTemperature of the…

Q: Calculate the pressure (in mmHg) exerted by methane, CH4, measured at 300. K, that can be produced…

A: Given data: Temperature T = 300 K Volume V = 604 L Mass of sugar = 1.50 kg = 1500 g Formula used: P…

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.