An "empty" container is not really empty if it contains air. How may moles of oxygen are in an "empty" two-liter cola bottle at atmospheric pressure (1 atm) and room temperature (25 °C)? Assume ideal behavior.
Express your answer to three significant figures and include the appropriate units.
The ideal gas law, PV = nRT is independent of the kind of gas. In other words, the pressure exerted by a given number of ideal gas particles is the same whether the sample consists of all one type of particle or a mixture of different kinds of particles.
Therefore, the pressure exerted by a mixture of gases can be expressed as follows:
A partial pressure is the pressure exerted by just one type of gas in a mixture. A partial pressure is calculated using only the number of moles of that particular gas, instead of the total number of moles:
The sum of the partial pressures is equal to the total pressure in the mixture:
Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules.
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