22.4 liters.
To calculate the volume of a gas, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin. Simply rearrange the equation to solve for V given the other variables. Alternatively, if the gas is at standard temperature and pressure (STP), you can use the molar volume of a gas at STP, which is 22.4 L/mol.
STP = Standard Temperature and Pressure After the IUPAC rules the standard temperature is 0 0C and the standard pressure is 100 kPa (0,986 atm). The molar volume of an ideal gas at STP is 22,710 980(38) L.
Well, darling, at standard conditions, 40 grams of argon gas would occupy approximately 22.4 liters. That's assuming you're talking about STP, where the pressure is 1 atmosphere and the temperature is 0 degrees Celsius. So, there you have it, 40 grams of argon gas takes up about as much space as a medium-sized beach ball.
The term used to indicate the space a weight of gas will occupy is called "volume." It refers to the amount of physical space that a gas occupies.
You can increase the volume of a gas by increasing the pressure applied to it. By compressing the gas into a smaller space, the gas particles will occupy a larger volume due to the increased pressure. This does not change the number or type of particles present in the gas.
1 mole of gas particles at STP (Standard Temperature and Pressure) occupies a volume of 22.4 liters.
Molar gas volume is the volume of ONE moel of gas. It only depends on the pressure and temperature, not on the kind of gas. Molar volume at standard temperature and standard pressure is always 22,4 Litres (for any gas)
The molar volume doesn't depend on the identity of the gas. One mole of any ideal gas at STP will occupy 22.4 liters.
The molar volume of hydrogen gas at STP (Standard Temperature and Pressure) is 22.4 liters per mole.
0.00922 g of H2 gas will occupy approximately 0.100 L at STP
The volume is approx. 15,35 litres.
The volume is 22,1 L.
PV=nRT 32 gram O2 = 1 mole O2 (1atm)(V) = (1 mole)(.0821)(273) V = 22.4 L
At STP (standard temperature and pressure: 0°C and 1 atm pressure), 1 mole of any gas occupies 22.4 liters. The molar mass of hydrogen gas (H2) is 2 g/mol. With 0.00919 g of H2, you have 0.004595 moles. So, at STP, it would occupy approximately 0.1029 liters, which is the same as 102.9 milliliters.
At RTP the assumed temperature is 293ºK, at STP the assumed temperature is 273ºK. The formula used for this is Pressure x Volume = moles x ideal gas constant x Temperature. So Volume = (moles x ideal gas constant x temperature) / Pressure Assuming Pressure and moles stays constant... Volume at RTP = ( 1 mole x 8.31451 x 293 K ) / ( 101.325 Pa) Volume at RTP = 24.0429 Volume at RTP = 24.0dm^3 Volume at STP = ( 1 mole * 8.31451 * 273 K ) / ( 101.325 Pa) Volume at STP = 22.4017 Volume at STP = 22.4dm^3
Molar volume = 22.4141 L/moleat standard temperature (melting ice) T = 273.15 K and standard pressure po= 1 ATM (= 1.01325*105 Pa)(At room temperature T=298 K and p=po the molar volume is 24.5 L/mole)
22.4 L. At STP 1 mole of any gas will always be equal to 22.4 L.