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Density is mass per volume. Density of gas is mostly the same in mol/volume. The molecular mass play large role in the different of density. Weak intermolecular force and interaction among different species of gases may give extra additional to the different in density of mix gas but at very small fraction.
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At stp the density of ccl4 vapours in g l will be neatest to?
At STP, the molar volume of any ideal gas is 22.4 L/mol. To find the density of CCl4 vapor at STP, we need to calculate its molar mass. CCl4 has a molar mass of 153.8 g/mol, so the density of CCl4 vapor at STP would be 153.8 g/mol divided by 22.4 L/mol, which equals approximately 6.86 g/L.
What is the relationship between the molar mass of a gas and its density?
The relationship between the molar mass of a gas and its density is that as the molar mass of a gas increases, its density also increases. This means that gases with higher molar masses will be denser than gases with lower molar masses.
What is the mass of 43.7 L of helium at STP?
The mass of 43,7 L of helium at STP is 7.8 g.
What is the mass of ethane gas inside a 5.00 L vessel at STP?
The molar volume of a gas at STP (Standard Temperature and Pressure) is 22.4 L. Ethane gas has a molar mass of 30.07 g/mol. Therefore, the mass of ethane gas in a 5.00 L vessel at STP can be calculated as (5.00 L / 22.4 L) * 30.07 g/mol.
Why is nitrogen gas at STP less dense than Xe gas at STP?
Nitrogen gas at STP is less dense than xenon gas at STP because nitrogen has a lower atomic mass and thus lighter molecules, leading to lower density. Additionally, xenon is a noble gas with a higher atomic mass and larger atomic radius, contributing to its higher density.
What is the vapour density of the gas if 5.6dm3of a gas weighs 60g at S.T.P?
The molar volume of a gas at STP (standard temperature and pressure) is 22.4 L/mol. To calculate the molar mass of the gas, you can use the formula: Molar mass = (mass of gas / volume of gas) x molar volume at STP. In this case, with a mass of 60g and a volume of 5.6 dm3, the molar mass would be 60g/5.6dm3 x 22.4L/mol = 240 g/mol. Vapour density is calculated as 2 x molar mass, so in this case the vapour density would be 480 g/mol.
Calculate the density of nitrogen gas, in grams per liter, at STP?
At Standard Temperature and Pressure (STP), which is defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere pressure, the molar volume of an ideal gas is approximately 22.4 liters/mol. The molar mass of nitrogen gas (N₂) is approximately 28.02 grams/mol. To calculate the density (D) of nitrogen gas at STP, you can use the ideal gas law: � = Molar mass Molar volume at STP D= Molar volume at STP Molar mass � = 28.02 g/mol 22.4 L/mol D= 22.4L/mol 28.02g/mol � ≈ 1.25 g/L D≈1.25g/L Therefore, the density of nitrogen gas at STP is approximately 1.25 grams per liter.
What is the density at STP of (H2S) in grams per liter?
At standard temperature and pressure (STP), the density of hydrogen sulfide (H₂S) is approximately 1.363 grams per liter. This value can be calculated using the molar mass of H₂S, which is about 34.08 g/mol, and the ideal gas law, considering that one mole of gas occupies 22.414 liters at STP. Therefore, the density is derived by dividing the molar mass by the volume at STP.
At stp the density of ccl4 vapours in g l will be neatest to?
At STP, the molar volume of any ideal gas is 22.4 L/mol. To find the density of CCl4 vapor at STP, we need to calculate its molar mass. CCl4 has a molar mass of 153.8 g/mol, so the density of CCl4 vapor at STP would be 153.8 g/mol divided by 22.4 L/mol, which equals approximately 6.86 g/L.
What is the relationship between the molar mass of a gas and its density?
The relationship between the molar mass of a gas and its density is that as the molar mass of a gas increases, its density also increases. This means that gases with higher molar masses will be denser than gases with lower molar masses.
What is the mass of 43.7 L of helium at STP?
The mass of 43,7 L of helium at STP is 7.8 g.
What is the density of a gas if its molar mass is 1.222 g?
At STP 1 mole of a gas occupies 22.4 L So D = m / V = 1.222g / 22.4 L = 0.0546 g/L This is the mathematical answer, but this is impossible. The lightest gas is Hydrogen with a molar mass of 2. No real gas is less than that.
What is the mass of ethane gas inside a 5.00 L vessel at STP?
The molar volume of a gas at STP (Standard Temperature and Pressure) is 22.4 L. Ethane gas has a molar mass of 30.07 g/mol. Therefore, the mass of ethane gas in a 5.00 L vessel at STP can be calculated as (5.00 L / 22.4 L) * 30.07 g/mol.
The volume of 1mole of hydrogen bromide at STP is 22.4 liters The gram-formula mass of hydrogen bromide is 80.9 grams per mole What is the density of hydrogen bromide at STP?
The molar volume of a gas at STP is 22.4 liters/mol. The molar mass of hydrogen bromide is 80.9 g/mol. Therefore, the density of hydrogen bromide at STP is 80.9 g/mol / 22.4 L/mol = 3.61 g/L.
What is the density of CO gas if G occupies a volume of ml?
To calculate the density of carbon monoxide (CO) gas, you need to know its molar mass, which is approximately 28.01 g/mol. Density (ρ) can be calculated using the formula ρ = mass/volume. If you have the volume of CO gas in milliliters (ml), you can convert it to liters (1 ml = 0.001 L) and then use the ideal gas law or the molar volume at standard temperature and pressure (STP) to find the mass. Once you have the mass, divide it by the volume in liters to find the density in g/L.
What is the weight of chlorine gas in lbs?
The weight of chlorine gas can vary depending on the volume and temperature. At standard temperature and pressure (STP), the molar mass of chlorine gas (Cl2) is approximately 70.91 grams/mol. To convert this to pounds, you would divide the molar mass by the conversion factor of 453.592 grams per pound. Therefore, the weight of chlorine gas would be approximately 0.156 pounds per mol at STP.
What is the mass of 39.6 dm3 of argon gas collected at STP?
The molar volume of any ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Converting 39.6 dm3 to liters gives 39.6 L. To find the mass of argon gas, we calculate the number of moles using the ideal gas equation (PV = nRT) and then multiply by the molar mass of argon.
