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.
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).
Firstly, an ideal gas is one consisting of identical particles with no volume. These particles feel no intermolecular forces and undergo perfectly elastic collisions with the all of the container. It is important to note that real gases do not exhibit these characteristics and that it merely provides an approximation. Though the heading "Ideal Gas" can be separated into two board sections, the classical thermodynamic ideal gas and the ideal quantum Boltzmann gas; from the question wording I'll assume it's the former we're dealing with (both are essentially the same, except that the classical thermodyamic ideal gas is based on classical thermodynamics alone). The classical ideal gas pressure, p, and its volume, V, are related in the following way: pV=nRT where n is the amount of gas in moles , R is the gas constant, 8.314J•K-1mol-1 (Joule Kelvin per mole) and T is the absolute temperature in Kelvin. Put simply : the relationship between pressure and volume is the that the change in pressure is inversly proportional to the volume. p= a/Vwhere a is a constant; in this case (nRT).
Pressure and volume are inversely proportional at any given temperature and quantity of molecules. Thus, a mole of gas squeezed into half the volume would have double the pressure if all other things remain equal. Conversely, a mole of gas whose pressure was halved would occupy double the volume, all other things remaining equal.
pressure = .490 atm
Vc is the specific volume (volume per mole) at the critical point of a substance. Vr is the "reduced volume" which is equal to the specific volume divided by the critical volume. Vr = V/Vc Many thermodynamic models correlate behavior of different substances in terms of their reduced volume. The principle of corresponding states indicates that substances at equal reduced pressures and temperatures have equal reduced volumes. This relationship is approximately true for many substances, but becomes increasingly inaccurate for large values of Pr. (Where Pr = P/Pc and Pc is the pressure at the critical point.)
Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the volume of 22.4 liters.
For Ideal gases, mole fraction=volume fraction
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
The volume varies inversely with pressure.
A mole of ideal gas at STP takes up 22.4 L.
Not sure what you mean by "first letter is a c", but the volume of one mole of an ideal gas at STP is 22.4 Liters.
The volume is 22,710 980(38) litres for the ideal gas.
This is the molar volume of an ideal gas at a given temperature and pressure.
1 mole of an ideal gas at STP occupies 22.4 liters. If STP is 'close' to the boiling point a real gas may deviate from ideal behavior and thus the volume will not be as predicted.
1 mole of an ideal gas at STP occupies 22.4 liters. If STP is 'close' to the boiling point a real gas may deviate from ideal behavior and thus the volume will not be as predicted.
I suppose that the correct anwer is 29,7 L.
Pressure, volume, temperature & the amount of gas.
i am almost positive it is 22.4 Liters per mole. The conversion for molecules to mole is 6.023 x 10^23 (avogadros number) and the relationship from grams to moles is dependant upon the molecular weight of the molecule you are talking about.