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The molar mass of a certain gas is 49 g. What is the density of the gas in gL at STP?
To find the density of a gas at standard temperature and pressure (STP), we can use the formula: density = molar mass / molar volume. At STP, the molar volume of an ideal gas is approximately 22.4 L. Therefore, the density of the gas with a molar mass of 49 g is calculated as follows: density = 49 g / 22.4 L ≈ 2.19 g/L.
What is the volume of 10.9 mol of helium at STP?
The volume of 10.9 mol of helium at STP is 50 litres.
Determine the volume of 76g of f2 at stp?
To find the volume of 76g of F2 at STP, we first need to determine the number of moles of F2 using the molar mass. The molar mass of F2 is 38 g/mol. 76g / 38 g/mol = 2 moles of F2. At STP, 1 mole of any gas occupies 22.4 L. Therefore, 2 moles of F2 would occupy 44.8 L at STP.
What is the mass or volume of one mole of water?
The molar mass of water (H2O) is approximately 18.015 grams per mole. The volume of one mole of water at standard temperature and pressure (STP) is about 18.0 milliliters.
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.
In what phase would a substance with a volume of 25.00mL and a mass of 78.05g be at STP?
Gas
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 volume at STP of a 49.6 gram sample of acetylene gas?
To find the volume of the acetylene gas at STP, we can use the ideal gas law equation: PV = nRT. First, we must convert the given mass of acetylene gas to moles using its molar mass. Then, knowing STP conditions (standard temperature = 273 K and standard pressure = 1 atm), we can calculate the volume.
The molar mass of a certain gas is 49 g. What is the density of the gas in gL at STP?
To find the density of a gas at standard temperature and pressure (STP), we can use the formula: density = molar mass / molar volume. At STP, the molar volume of an ideal gas is approximately 22.4 L. Therefore, the density of the gas with a molar mass of 49 g is calculated as follows: density = 49 g / 22.4 L ≈ 2.19 g/L.
What is the volume of 10.9 mol of helium at STP?
The volume of 10.9 mol of helium at STP is 50 litres.
Determine the volume of 76g of f2 at stp?
To find the volume of 76g of F2 at STP, we first need to determine the number of moles of F2 using the molar mass. The molar mass of F2 is 38 g/mol. 76g / 38 g/mol = 2 moles of F2. At STP, 1 mole of any gas occupies 22.4 L. Therefore, 2 moles of F2 would occupy 44.8 L at STP.
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 volume of 11 g of SO2 at STP conditions?
At STP conditions (standard temperature and pressure), the volume occupied by 1 mole of ideal gas is 22.4 liters. Since the molar mass of SO2 is approximately 64 g/mol, 11 g of SO2 is about 0.172 moles. Therefore, the volume of 11 g of SO2 at STP would be approximately 3.85 liters.
What is the mass or volume of one mole of water?
The molar mass of water (H2O) is approximately 18.015 grams per mole. The volume of one mole of water at standard temperature and pressure (STP) is about 18.0 milliliters.
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.
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 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.
