The mole fraction of Oxygen = 21/100= .21
The chemical equation for hydrogen gas and oxygen gas combining to form water is as follows: 2H2 (g) + O2 (g) ---> 2H2O (l). This means that for every 1 mole of oxygen gas reacting, two moles of hydrogen gas are needed. So if 0.50 moles of oxygen gas react to form one mole of water, then one mole of hydrogen gas was used.
find the mole fraction on each: Mole fraction gas (X) = moles of gas (X) / total moles of all gases Then use this formula: Pi = X Pt Where Pi = partial pressure of gas i X = mole fraction of gas i Pt = total pressure of all gases How do you calculate the total pressure?Is it just the total number of moles?Or do you need to convert it to Pascals?
For any gas, at most temperatures and pressures, the number of particles in a given volume is the same (based on the Ideal Gas Law -- see the Related Questions to the left for more information). The density is defined as the mass divided by volume, and therefore the density of a gas depends only on the mass of the particles. Since molecular oxygen is heavier than the average weight of air, which is largely composed of molecular nitrogen (which is lighter) and molecular oxygen, then oxygen is denser than air.Based on the composition of air (see the Related Questions to the left), the average molecular weight of air is 28.97 grams per mole (which is dominated by the molecular weight of N2, which is 28.0134 g/mole because the atmosphere is nearly 80% N2). The molecular weight of oxygen, O2, is 32.0 grams per mole which is just slightly heavier. Therefore, oxygen is just slightly more dense than air, but not by much. In comparison, the molecular weight of helium, He, is only 4.003 g/mole, which is much lighter than air!~air is made up of nitrogen, oxygen, argon, and carbon dioxide
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