If air contains 78% of nitrogen by volume, what is the solubility of nitrogen in water at 298K ?
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To determine the solubility of nitrogen in water at 298K, we can use Henry's law, which states that the solubility of a gas is directly proportional to its partial pressure.
First, we need to determine the partial pressure of nitrogen in air. Given that air contains 78% nitrogen by volume, we can assume that the partial pressure of nitrogen is also 78% of the total pressure of air.
Therefore, the partial pressure of nitrogen (PN2) can be calculated as follows:
PN2 = 78% x Ptotal
Next, we'll use the solubility of nitrogen in water at 298K, which is the Henry's law constant. This value varies depending on the source, but for simplicity, we'll use an approximate value of 1.34 x 10^-3 mol/(L·atm) as a general estimate.
Lastly, we can use Henry's law to determine the solubility of nitrogen in water at 298K:
Solubility of nitrogen (SN2) = Henry's Law Constant x PN2
Keep in mind that Henry's law assumes ideal behavior, so it may not be entirely accurate. However, for approximate calculations, this formula should be sufficient.