The molar volume of an ideal gas at 25 0C and 100 kPa is 0,875 436 4 cubic feet.
22.4
22.4ft^2
Gases are not measured by linear measures such as feet or meters - they are measured either by mass (pounds, kilograms), or by volume (liters, cubic feet). In the case of a volume, you must also know the pressure.
The atomic volume of carbon is 5.31 cubic centimeters per mole at room temperature and pressure.
The atomic mass of zinc is approximately 65.38 g/mol. Therefore, one mole of zinc would weigh 65.38 grams.
NaHO 55.5
1 mole of gas particles at STP (Standard Temperature and Pressure) occupies a volume of 22.4 liters.
Gases are not measured by linear measures such as feet or meters - they are measured either by mass (pounds, kilograms), or by volume (liters, cubic feet). In the case of a volume, you must also know the pressure.
The molar volume, symbol Vm,[1] is the volume occupied by one mole of a substance (chemical element or chemical compound) at a given temperature and pressure. It is equal to the molar mass (M) divided by the mass density (ρ). It has the SI unit cubic metres per mole (m3/mol),[1] although it is more practical to use the units cubic decimetres per mole (dm3/mol) for gases and cubic centimetres per mole (cm3/mol) for liquids and solids.
Measure the length of the room. We'll call this length "L" Measure the width of the room. We'll call this width "W" Measure the height of the room. We'll call this height "H" Volume = L * W * H
The exact amount of Brown's gas produced will depend on the efficiency of the electrolysis process and the volume of hydrogen and oxygen gases that are generated. However, typically, one gallon of water (which is approximately 0.1337 cubic feet) can produce about 1800 gallons of Brown's gas at standard temperature and pressure.
One pound = 0.453592kg. One Mole of H = 1g 0.453592kg of H = 453.592 mole of H According to the ideal gas law, one mole of gas will occupy 22.4 liters as stp. One pound of H will occupy 10,160.2608 liters, or 358.806 cubic feet. Be careful. Most applications of this calculation will deal with hydrogen gas, which has two hydrogen atoms per molecule at standard temperature and pressure. In such cases, divide the volume calculated above by two.
For solids and liquids, if you know the density in grams per cubic centimeter, and the atomic mass (grams per mole), then you can calculate it. Moles * (atomic mass) / (density) = volume. For gasses: you need to know the Pressure and Temperature, and use PV = nRT, so V = n*R*T/P, then convert to cubic centimeters. Or if at Standard Temperature and Pressure (0°C and 1 atmosphere), an Ideal Gas has a volume of 22.4 liters/mole (22400 cm3 / mole)
One Mole
For Ideal gases, mole fraction=volume fraction
Mole is not a unit of volume. Mole deals with numbers like dozen.
If ounce-mole - in ounces if pound-mole - in pounds and so on
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
Mass of 1 mole hydrogen gas (H2) = 2 grams. So the mass of 22.4 liters (stp) H2 is 2 g. 1 kilogram = 1kg = 1000 grams. 1 cubic foot = 28.25 liters 1000 grams of H2 = 500 X 28.35 liters = 11,200 liters 11,200 liters = 396.460177 cubic feet Answer = ~396.5 cubic feet = Bonus answer - 14.68 cubic yards http://www.siei.org/usefulequations.html