Yes - as long as the pressure and temperature are constant.
the mole fraction of oxygen= 37/100 0.37 the mole fraction of Nitrogen= .63 that equals to give 1
1 mole of a gas at S.T.P always has the volume 22.414dm3 so number of moles multiply by 22.414 (molar volume) is equal to total volume at S.T.P , volume at other conditions may be calculated by equation of states, P1V1/T1 = P2V2/T2
A mole of ideal gas at STP takes up 22.4 L.
molar volume
The volume occupied by 1 mole of diatomic gas particle at NTP ( Normal Temperature & Pressure) is 11.2 L
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
22.4 L. At STP 1 mole of any gas will always be equal to 22.4 L.
Oxygen is the second most common/abundant gas in the air that we breathe. Nitrogen is the most abundant gas in the air we breathe. The composition of air is often treated as 79 mole or volume percent N2 and 21 mole or volume percent O2.
Oxygen is the second most common/abundant gas in the air that we breathe. Nitrogen is the most abundant gas in the air we breathe. The composition of air is often treated as 79 mole or volume percent N2 and 21 mole or volume percent O2.
the mole fraction of oxygen= 37/100 0.37 the mole fraction of Nitrogen= .63 that equals to give 1
1 mole of a gas at S.T.P always has the volume 22.414dm3 so number of moles multiply by 22.414 (molar volume) is equal to total volume at S.T.P , volume at other conditions may be calculated by equation of states, P1V1/T1 = P2V2/T2
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 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.
A mole of gas is equal to 6.02 x 1023 gas molecules.
1 mole of every gas has a volume 22.414 dm3 at S.T.P.
A mole of ideal gas at STP takes up 22.4 L.
molar volume