A 248-mL gas sample has a mass of 0.433 g at a pressure of 745 mmHg and a temperature of 28 °C. What is the molar mass of the gas?

Q: An experiment shows that a 268 mLmL gas sample has a mass of 0.428 gg at a pressure of 755 mmHgmmHg…

A: A gas sample has, Mass =  0.428 g Volume = 268 mL Pressure = 755 mmHg Temperature =  38°C,

Q: If the pressure exerted by a gas at 25°C in a volume of 0.057 L is 3.80 atm, how many moles of gas…

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Q: A 14.62 mol sample of argon gas at 27.58 °C occupies 28.68 L. What is the pressure in kPa? Provide…

A: Pressure of argon gas is calculated using ideal gas equation PV=nRT.

Q: If a 2.29-g sample of a gas occupies 750. mL at STP, what is the molar mass of the gas at 125oC?

A: An ideal gas is a potential gas consisting of several particles of random motions not…

Q: If a gaseous mixture is made of 2.41g of He and 2.79g of Ne in an evacuated 1.04-L container at 25…

A: The volume of a container is 1.04 L. The given weight of He is 2.41 g.The given weight of Ne is 2.79…

Q: If the density of an ideal gas at STP is found to be 0.0902 g/L., what is its molar mass? molar…

A: The given data is as follows: The density of the ideal gas at STP = 0.0902 g/L The molar mass of the…

Q: How many moles of CO2 are there in a 46.0 L sample of the gas at a pressure of 0.9 atm and a…

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Q: A large tank is filled with 125 mol O₂ to a pressure of 2245 torr at 25.0 °C. What is the volume (in…

A: The ideal gas equation is  PV = nRT  P = pressure  V = volume  n = moles of gas  R = gas constant =…

Q: What volume is occupied by 12.5 g of argon gas at a pressure of 1.05 atm and a temperature of 322 K?…

A: Given: volume of Ar = 12.5 g pressure of Ar = 1.05 atm temperature of Ar = 322 K volume of He =…

Q: Calculate the molar mass of a gas that has a density of 1.70 g/L at STP

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Q: What volume is occupied by 20.3 g of argon gas at a pressure of 1.47 atm and a temperature of 449 K?…

A: According to ideal gas equation, PV = nRT Therefore, Assuming this to be an ideal gas , The volume…

Q: What is the volume (in mL) of a sample of 87.4 g of Cl2 gas that has a temperature of −22°C and a…

A: The given data contains, mass = 87.4 g. Temperature = 251 K. Pressure = 993 torr.   = 1.306 atm.

Q: A 3.55 g sample of an unknown gas at 23 ∘C and 1.05 atm is stored in a 3.05 L flask. What is the…

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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: What pressure in atmospheres corresponds to 720.3mm Hg?

A: We have to convert the unit of given pressure (720.3 mmHg) from mmHg to atmosphere.

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: A 113-mL gas sample has a mass of 0.171 g at a pressure of 721 mmHg and a temperature of 32 °C. What…

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Q: How many moles of gas are present with a volume of 25 L, a pressure of 105 kpa and a temperature of…

A: Using ideal gas equation, we have P*V=n*R*T         --------(1) where, P is pressure  V is volume R…

Q: Under a pressure of 862 kPa, a gas has a volume of 752 mL. The pressure is increased, without…

A: As the concentration of the gas and the temperature of the system remains constant, Boyle's law can…

Q: If the pressure exerted by a gas at 100°C in a volume of 0.044 L is 3.81 atm, how many moles of gas…

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Q: If 0.370 L of neon gas is collected over water at a temperature of 60°C and a pressure of 760 torr,…

A: GIVEN: The volume of Neon gas collected over water= 0.370 L Temperature =60°C  Pressure = 760 torr…

Q: A 4.05 g sample of an unknown gas at 33 °C and 1.05 atm is stored in a 3.05 L flask. What is the…

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Q: Calculate the temperature at which a 2.00 L sample of gas at 27oC would occupy 3.00 L if its…

A: Given that =  Initial volume (V1) = 2.00 L Final volume (V2) = 3.00 L Initial temperature = 27°C =…

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: If the pressure exerted by a gas at 25°C in a volume of 0.044 L is 3.81 atm, how many moles of gas…

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

Q: A 1.75 g sample of an unknown gas at 47 C and 1.00 atm is stored in a 1.85 L flask. What is the…

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Q: If 0.600 g of a gas occupies 198 mL  at 30 C  and 665 mmHg  of pressure, what is the molar mass of…

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Q: What is the molar mass of a gas if 0.0494 g of the gas occupies a volume of 0.100 L at a temperature…

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Q: What volume is occupied by a 1.83 mol sample of nitrogen gas at a temperature of 0 °C and a pressure…

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Q: A sample of gas at 911.9 mmHg and occupying a volume of 13.20 L has a decrease in pressure to 98.94…

A: We have to calculate the new volume.

Q: Calculate the mass of 6.2 L of CO2 at 300° K and a pressure of 758.0 mm Hg.

A: CO2 gas Volume = V = 6.2 L Temperature = T = 300 K Pressure = P = 758.0 mm Hg ( 1 atm = 760 mm Hg )…

Q: What is the volume of this sample?

A: Ideal Gas Law :-  PV = nRT  P is the pressure of gas  V is the volume occupied by gas n is the…

Q: What is the density of sulfur dioxide gas at 795 torr and 25 oC?

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Q: g/mol. The molecular weight of a gas that has a density of 4.1 g/L at STP is

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Q: What is the total pressure in mmHg of a gas mixture containing: 0.25 atm of argon, 350 mmHg of He,…

A: Given:Pressure of He = 350 mmHg = 0.4605 atmPressure of Ar = 0.25 atm.Pressure of N2 = 0.47368421…

Q: In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605.6 mmHg and 21.6oC, it is…

A: Given information:Volume = 12.8 LPartial pressure of chlorine = 143 mmHgPressure = 605.6…

Q: If 5.0 moles of O2 and 3.0 moles of N2 are placed in a 30.0 L tank at a temperature of 25° C, what…

A: Moles of O2 gas and moles of N2 gas is given and finale volume and temperature is given . Total…

Q: Calculate the density of Xenon gas at a pressure of 742 mmHg and a temperature of 450C. The molar…

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Q: What is the molar mass of a gas if 0.281 g of the gas occupies a volume of 125 mL at a temperature…

A: Given, amount of gas =0.281 gvolume of gas =125 mL =0.125 Ltemperature =126 °C  =(126+273.15) K…

Q: If 0.275 moles of oxygen gas are held in a sealed 550 mL flask at a pressure of 800 mm, what is the…

A: Given, Moles of Oxygen gas (n) = 0.275 moles Note: 1000 mL= 1L Volume of a gas (V) = 550 mL = 0.550…

Q: The molecular weight of a gas that has a density of 6.75 g/L at STP is __________ g/mol.

A: At stp pressure is one atm

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: Calculate the volume of a sample of an ideal gas that contains 5.58 mol at 738 mmHg and 0°C.

A: Following information given in the question - Moles of the gas = 5.58 mol Pressure = 738 mmHg…

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: Assuming that a 800 mg gas occupying a volume of 1,100 ml at a pressure of 1,600 mmHg and a…

A: Volume = 1100ml = 1.1L  Pressure = 1600 mmHg = 2.1052 atm  T = 75oC =  75 + 273K = 348K  Gas…

Q: At 24 °C and 745 mmHg, the density of an unknown gas is determined to be 7.76 g/L. What is the molar…

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Q: What mass of neon gas is required to fill a 5.52-L container to a pressure of 1.17 atm at 37…

A: Use the ideal Gas equation to calculate the moles of Gas, Then using moles calculate the mass of the…

Q: Calculate the density of xenon gas at a pressure of 742 mmHgmmHg and a temperature of 45 ∘C

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Q: What is the pressure of a 8.0 g sample of nitrogen gas at 25 degress celcius in a closed 500 mL…

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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.