At 35.0 °C, a 12.0 L vessel is filled with 6.25 moles of Gas A and 6.00 moles of Gas B. What is the total pressure?

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 5.00 moles of Gas B. What is the…

A: Given-> Temperature (T) = 25.0°C = 25.0 + 273 = 298 K Volume of vessel (V) = 10.00 L Moles of A =…

Q: A mixture containing 0.765 mol He(g), 0.330 mol Ne(g), and 0.110 mol Ar(g) is confined in a 10.00-L…

A: Given  No. Of moles of He = 0.765 mol No. Of moles of Ne = 0.330 mol No. Of moles of Ar = 0.110 mol…

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: At 25.0° C, a 10.00 L vessel is filled with 7.00 atm of Gas A and 5.89 atm of Gas B. What is the…

A: The partial pressure is the mixture of gases being occupied the with same volume at the same…

Q: At 25.0° C, a 10.00 L vessel is filled with 6.30 atm of Gas A and 7.89 atm of Gas B. What is the…

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Q: At 0 degrees C, a 1.0-L flask contains 5.0×10−2 mol N2, 1.5×102 mg O2, and 5.0×1021 molecules of…

A: Given, volume of flask V =1.0 Ltemperature T =0°C =273.15 Knumber of moles of N2 =5.0×10-2 mol =0.05…

Q: A sample of oxygen gas, which is saturated with water vapour, is kept in a 10 L vessel at 30° C and…

A: Given, Total pressure, (PO2 + PH2O) = 758 Torr Pressure of water vapor, (PH2O) = 31.8 Torr

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: At 45.0 °C, a 14.0 L vessel is filled with 7.25 moles of Gas A and 4.20 moles of Gas B. What is the…

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Q: Since helium is lighter than air, it is difficult to measure the mass of a sample, so to find out…

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Q: To what volume would you have to change 6.5 liters of a gas at 1.25 atm in order to decrease its…

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Q: A 3.35 g sample of an unknown gas at 23 C and 1.10 atm is stored in a 3.05 L flask. What is the…

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Q: What final pressure must be applied to a sample of gas having a volume of 200. mL at 20.0°C and 750.…

A: Initial volume = 200 ml  Initial temperature = 20°C   Initial pressure = 750 torr Final volume = 600…

Q: A 2.55 g sample of an unknown gas at 31 ∘C and 1.05 atm is stored in a 2.85 L flask. What is the…

A: First the density is determined by using density formula as shown below,

Q: A quantity of CO gas occupies a volume of 0.48 L at 1.0 atm and 275 K. The pressure of the gas is…

A: From ideal gas law PV = nRT , where P = 1atm, T = 275 K , V = 0.48 L , n = moles of CO n = PV / RT…

Q: A gas mixture contains each of the following gases at the indicated partial pressures N 2 ,216 torr;…

A: Partial pressure of N2 = 216 torr ...Or  because 1 atm = 760 torr  ...so,  = 216 torr × (1 atm / 760…

Q: At 25.0 ° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.60 moles of Gas B. What is…

A: According to the ideal gas law, we know that  PV = nRT Where  P = pressure of the gas V = volume of…

Q: The density of a sample of gas is 1.00 g/L at 745 mmHg and 109°C. What is the molar mass of the gas

A: The ratio of mass per volume of a given substance is called its density. The equation of state of a…

Q: At 304.8 K, a 9.58 L tank contains 1.90 moles of H2 gas under a certain pressure in atm. Calculate…

A: Given, Volume = 9.58 L Number of moles = 1.90 mol Temperature = 304.8 K

Q: An 8.00-g sample of a gas occupies 22.4 L at 2.00 atm and 273 K. What is the molar mass of the gas?

A: Given that -  Mass of the gas = 8.00 g  Volume of the gas = 22.4 L  Pressure of the gas = 2.00 atm…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 5.95 moles of Gas B. What is the…

A: Given, volume of vessel =10.00 Ltemperature =25°C =(25+273) K =298 Knumber of mole of gas A =5.25…

Q: 2. A mixture of 6.0 g O2(g) and 9.0 g CH49) is placed in a 15 L vessel at 0 C. What is the partial…

A: Dear student ,   since you have posted multiple questions we will allow to solve only first question…

Q: What is the temperature, in K, of a 1.0 mole sample of gas that initially had a pressure of 1.01…

A: The final pressure in the atm is determined as follows. P2=767.6 torrP2=767.6 torr760 torr/atm=1.01…

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: If the mercury in a manometer raises 30.0 millimeters due to a change in pressure, what is the…

A: Mercury manometer raises=30.0 mm Pressure (in atm)=? 1 atmosphere (atm) = 760 millimeters of Hg…

Q: A mixture of three gases has a total pressure of 1380. mm Hg at 298 K. The mixture is analyzed and…

A: Given :  total pressure = 1380 mm Hg  number of moles of CO2 = 1.27 mol  number of moles of CO =…

Q: At 25.0 ° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.10 moles of Gas B. What is…

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Q: A 1.95 g sample of an unknown gas at 67 °C and 1.05 atm is stored in a 2.05 L flask. What is the…

A: The molar mass of a chemical compound is defined as the mass of a sample of that compound divided by…

Q: A sample of an unknown gas weighing 10.9 g occupies a 25.585 L container at a pressure of 0.694 atm…

A: Given a sample of gas,mass of gas =10.9 gvolume of gas =25.585 Lpressure of gas =0.694 atmand…

Q: If 4.81 g Ar are added to 4.01 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: First Calculate mole of Ar by mass÷molar mass Then Mole of He by PV=nRT. After this for total…

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: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 5.00 moles of Gas B. What is the…

A: According to ideal gas law PV = nRT where P = total pressure V = volume of vessel n = total moles R…

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: A gas mixture contains each of the following gases at the indicated partial pressures: N2, 226 torr…

A: Given:The pressures of three gases,N2 = 226 torrO2 = 125 torr  He = 109 torrWe need to calculate the…

Q: If 3.87 g Ar are added to 2.64 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: The number of moles of argon is calculated as follow 1 mole of argon = 39.95 g X mole of argon =…

Q: At what temperature will a 4.0 g sample of neon gas exert a pressure of 507 torr in a 6.0 L…

A: Solution: The ideal gas law is, where, P =the pressure of gas. V= volume of the gas n = number of…

Q: A balloon with a 2.00 L volume contains 1.10 moles of gas. How many moles would have to be released…

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

Q: For a gas sample whose total pressure is 740 torr, what are the partial pressures if the moles of…

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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: 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: At 25.0° C , a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.10 moles of Gas B. What is…

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Q: Consider three 1-L flasks at STP. Flask A contains NH3 gas, flask B contains NO2 gas, and flask C…

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Q: If 1.79 g Ar are added to 1.18 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

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Q: How many moles of a gas at 100.0 °C does it take to fill a 1.00 L flask to a pressure of 1,50 atm?

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Q: If 42.5 g of O2 and 2.8 g of CO2 are placed in a 11.2 L container at 24 °C , what is the pressure of…

A: Given mass of O2 = 42.5 g  mass of CO2 = 2.8 g volume = 11.2 L temperature = 24 °C

Q: A mixture of He, Ne and Ar has a total pressure of 4.55atm and is found to contain 0.22mol He,…

A: Partial Pressure Total pressure of a system is the sum of pressure of all the individual gas.…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 8.30 moles of Gas B. What is the…

A: It is given that the temperature is 25°C and the volume of the vessel is 10.00 L and the moles of…

Q: At 1.29 atm and 29.54∘C, a 3.14 g sample of gas occupies a volume of 1.70 ×103 mL. Calculate the…

A: Given, P= 1.29 atm  Mass = 3.14 g Volume = 1.70 ×103 mL T = 29.54∘C

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.55 moles of Gas B. What is the…

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Q: A 1.05 g sample of an unknown gas at 61 "C and 1.05 atm is stored in a 2.55 L flask. What is the…

A: Mass per unit volume is known as density. S.I unit of density is g/cm3 or kg/m3. Other units of…

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.