Do equal volumes of gases contain the same number of molecules?
Avogadro’s law, a statement that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules. This empirical relation can be derived from the kinetic theory of gases under the assumption of a perfect (ideal) gas.
How is it possible that all gases have the same volume at the same temperature and pressure?
A modern statement is: Avogadro’s law states that “equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.” For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.
Why can equal volumes of gases at standard pressure and temperature have to contain equal numbers of particles?
Avogadro’s hypothesis states that equal volumes of all gases at the same temperature and pressure contain equal numbers of particles. Since the total volume that a gas occupies is made up primarily of the empty space between the particles, the actual size of the particles themselves is nearly negligible.
What relationship exists between the volume and the number of moles of a gas?
Avogadro’s Law
A plot of the effect of temperature on the volume of a gas at constant pressure shows that the volume of a gas is directly proportional to the number of moles of that gas. This is stated as Avogadro’s law.
Why do all gases occupy the same volume?
Why do all gases have the same molar volume at STP?
As all gases that are behaving ideally have the same number density, they will all have the same molar volume. At STP this will be 22.4 L. This is useful if you want to envision the distance between molecules in different samples.
What is the relationship between the number of gas particles and volume are these two variables directly proportional or do they vary inversely?
The volume of a given gas sample is directly proportional to its absolute temperature at constant pressure (Charles’s law). The volume of a given amount of gas is inversely proportional to its pressure when temperature is held constant (Boyle’s law).
What is the relationship between the amount of gas indicated by moles and volume directly or indirectly proportional?
At constant temperature and pressure the volume of a gas is directly proportional to the number of moles of gas.
Do all gasses occupy the same volume?
Only ideal gases are guaranteed to occupy 22.4 L/mol at STP. There are many gases that are not ideal. So going by this, all gases should occupy same x L at some other temperature-pressure conditions.
Does gas stay the same volume?
Gas is a state of matter that has no fixed shape and no fixed volume. Gases have lower density than other states of matter, such as solids and liquids.
Do all gases have the same volume at STP?
How are the volumes to two different gases both at STP similar?
If both gases are at STP, they share the same temperature and system pressure, and if the same number of particles of each gas are in the closed container, then the only variable left is their volumes.
Why do the equal volumes of any gases have equal number of molecules?
According to Avogadro’s hypothesis, why do the equal volumes of any gases have an equal number of molecules at constant temperature and pressu… It is known that equal volumes of all gases contain equal number of molecules under similar conditions of temperature and pressure .
How many molecules are there in one mole of gas?
One mole of any gas contains the same number of molecules (Avogadro’s Number), The kinetic theory shows that the product PV is proportional to the number of molecules with no reference to size. technically “in the limit of zero pressure and infinite temperature.”
Do molecules of different gases have different sizes?
“molecules of different gases have a different size, so, when tightly packed, the same number of molecules should take different volumes.” The logic is OK; the first premise about different sizes is only partially OK , the second premise isn’t OK at all.
How does molar mass affect the volume of an ideal gas?
The equation shows that, as the number of moles of gas increases, the volume of the gas also increases in proportion. Similarly, if the number of moles of gas is decreased, then the volume also decreases. Thus, the number of molecules or atoms in a specific volume of ideal gas is independent of their size or the molar mass of the gas.