To find it's density
10 kg is mass = STP = 10 ltr volume
The volume of 10.9 mol of helium at STP is 50 litres.
Density is the amount of mass per given volume, thus the formula for density of an object with a known mass and volume is as follows: ρ=m/V where: ρ - (rho) Density (Kg m-3) m - Mass (Kg) V - Volume (m3)
One mole has amass of 16g.There are 6.428mol.Its mass is 102.85g
Most commonly, this refers to the volume of a gas at Standard conditions of Temperature and Pressure (often abbreviated, STP). This standard allows accurate comparisons of volumes. The volume of a gas (any gas) at STP is 22.4 liters per mole.
Gas
10 kg is mass = STP = 10 ltr volume
Acetylene is C2H2, with a molar mass of 26g/mol. 49.6g of it = 1.9 moles. At STP, 1 mole of any gas occupies a volume of 22.4 liters, so 1.9 moles at STP would have a volume of 42.56 liters.
atoms have a higher mass than molecules. Because both gases at STP have the same number of molecules per unit volume, the gas must be denser.
The volume of 10.9 mol of helium at STP is 50 litres.
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.
Density is the amount of mass per given volume, thus the formula for density of an object with a known mass and volume is as follows: ρ=m/V where: ρ - (rho) Density (Kg m-3) m - Mass (Kg) V - Volume (m3)
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 (Nā) is approximately 28.02 grams/mol. To calculate the density (D) of nitrogen gas at STP, you can use the ideal gas law: ļæ½ = Molar mass Molar volume at STP D= Molar volume at STP Molar mass ā ļæ½ = 28.02 ā g/mol 22.4 ā L/mol D= 22.4L/mol 28.02g/mol ā ļæ½ ā 1.25 ā g/L Dā1.25g/L Therefore, the density of nitrogen gas at STP is approximately 1.25 grams per liter.
The mass of 43,7 L of helium at STP is 7.8 g.
3.61g/L D=m/v
One mole has amass of 16g.There are 6.428mol.Its mass is 102.85g
1 standard volume of 1 mole of any gas @ STP is 22.4 LSo the # of moles in a 1 L sample will be:1 L*(1 mol/22.4 L) = 0.04464 molSince you already know the mass of the gas @ STP, the molar mass will be mass/#moles1.92 g/ 0.04464 mol = 43.01 g/mol