On a clear day at sea level, the partial pressure of N2 in air is 0.78 atm at 25 degres C. Under these conditions, the concentration of N2 in water is

5.3 x 10^-4 M. What is the partial pressure of N2 when the concentration in water is 3.5 x10^-4 M?

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To determine the partial pressure of N2 when the concentration in water is 3.5 x 10^-4 M, we need to use Henry's Law, which relates the concentration of a gas in a liquid to its partial pressure.

Henry's Law equation is given as:

C = k * P

Where:
C is the concentration of the gas in the liquid (in Molarity, M)
k is the Henry's Law constant for the specific gas-solvent pair
P is the partial pressure of the gas in the gas phase (in atm)

In this case, we have the concentration of N2 in water, which is 5.3 x 10^-4 M at a certain partial pressure of N2 in the gas phase, which is 0.78 atm.

So, we can rearrange Henry's Law equation to solve for P:

P = C / k

To find the partial pressure of N2 when the concentration in water is 3.5 x 10^-4 M, we need to know the Henry's Law constant (k).