100
-Ivin
0.44g\2=0.22mol 0.22*22.4=4.928dm3
31.8 L
The answer is 445.088 .
One mole has a volume of 22.4l.So the volume is 224ml
STP (standard temperature and pressure)
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
The volume of 10.9 mol of helium at STP is 50 litres.
31.8 L
The volume is 695,62 cm3.
The volume is 695,85 cm3.
The answer is 445.088 .
The volume of 5.0 moles of 02 at STP is 100 litres.
1 mol of any gas has a volume of 22.4 L at STP
One mole has a volume of 22.4l.So the volume is 224ml
STP (standard temperature and pressure)
The volume is 22,1 L.
At STP, 1 mole of an ideal gas occupies 22.4 liters. 0.335 mol x 22.4 L = 7.50 L .................. 1 mol
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.