The volume of any gas at STP is 22.4 liters/mole. Thus, 41.6 moles x 22.4 L/mole = 931.84 liters, or
932 liters (to 3 sig figs).
The molar volume of the ideal gas at 1 at and 0 oC is 22,414 L; this is a law in chemistry, extended also to real gases.
22,414 x 41,6 = 932,4 L
This volume is 79,79 litres.
One mole has amass of 16g.There are 6.428mol.Its mass is 102.85g
The volume of 10.9 mol of helium at STP is 50 litres.
I mole - 16g of methane is 1 mole. At STP it would occupy 22.4 liters
0.25 moles
This volume is 79,79 litres.
How many molecules are in 30 liters of methane (CH4) at STP
One mole has amass of 16g.There are 6.428mol.Its mass is 102.85g
first, convert the 0.416g into moles. o.416/83.80 = 0.0050mol second, since there is 1 mol for 22.4L at STP, you write: 0.0050mol x (22.4L / 1mol) and your answer: 0.1112L
The volume of 10.9 mol of helium at STP is 50 litres.
I mole - 16g of methane is 1 mole. At STP it would occupy 22.4 liters
0.25 moles
Use PV =nRT ( pressure at STP is 1 atmosphere and temp. is 298.15 Kelvin ) (1 atm)(volume) = (1.50 mole)(0.08206 Latm/molK)(298.15 K) = 36.7 Liters
24.5
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 amount of oxygen is 0,067 moles.
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.