6 litre of o2 in equivalent to how many moles
Answers
Answer:
The Ideal Gas Law predicts very precisely not only gas volume, but temp and the number of moles of gas. To do this, it makes some assumptions about the behavior of a gas, which is where the “ideal” part comes from. At standard temperature and pressure (STP), one mole of an ideal gas takes up 22.7 liters (updated in the 1980s from 22.4 L when IUPAC changed the definition of STP to 1 bar (100 kPa) nstead of 1 atmosphere (103.1 kPa). You can solve for volume of gas by using the formula PV = nRT where P = pressure in atmospheres, V is volume in liters, n is the number of moles of gas, R is the gas constant 0.082 and T is temperature in degrees Kelvin (K).
So, as P rises, either V or T must decrease. If you have the gas in a sealed bottle (volume is constant, as P rises, T must also rise to keep the two sides of the equation in balance. But a picture is worth a 1000 words …
So at STP (273.15 K, or 0 C), the volume of one mole of an ideal gas at STP would be:
V = nRT / P (same formula as before, but solving for V)
Substituting in the values for one mole of gas at STP gives us: V = 1 mole * (0.082 * 273.15) / 0.987Atm = 22.7 L
Here is an image that shows what it would look like if we could see gas molecules at low vs. high pressure. Here, the number of moles of gas is held constant but the volume is reduced, causing an increase in pressure. Note that pressure is simply the sum of the force of all the gas molecules impacting each square centimeter of the side of the container.
Answer:
The Ideal Gas Law predicts very precisely not only gas volume, but temp and the number of moles of gas. To do this, it makes some assumptions about the behavior of a gas, which is where the “ideal” part comes from. At standard temperature and pressure (STP), one mole of an ideal gas takes up 22.7 liters (updated in the 1980s from 22.4 L when IUPAC changed the definition of STP to 1 bar (100 kPa) nstead of 1 atmosphere (103.1 kPa). You can solve for volume of gas by using the formula PV = nRT where P = pressure in atmospheres, V is volume in liters, n is the number of moles of gas, R is the gas constant 0.082 and T is temperature in degrees Kelvin (K).