The solubility of nitrogen gas in water at 25 °C and 1 atm is
6.8!10"4 mol/L. If the partial pressure of nitrogen gas in air above water is 0.76 atm, what is the concentration of dissolved nitrogen?
see your post 2-3 pages closer to the top.
To find the concentration of dissolved nitrogen, we need to use Henry's Law, which states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Henry's Law equation can be written as:
C = k * P
Where:
C is the concentration of the gas in the liquid (mol/L)
k is Henry's Law constant (mol/(L·atm))
P is the partial pressure of the gas above the liquid (atm)
We can rearrange the equation to solve for the concentration C:
C = P/k
To find the concentration of dissolved nitrogen, we need to know the Henry's Law constant, k, for nitrogen gas in water at 25 °C. However, this value is not provided in the question. Without this information, we cannot calculate the concentration of dissolved nitrogen accurately.
Therefore, we need additional data to determine the Henry's Law constant, k, specific to nitrogen gas in water at 25 °C.