The Henry’s Law constant for N2 in water at 30 oC is 6.0 x 10-4 M/atm, calculate the

solubility of nitrogen gas in water at a partial pressure of 2.5 atm

See your post above. Same formula.

To calculate the solubility of nitrogen gas (N2) in water at a partial pressure of 2.5 atm, we can use Henry's Law. Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

The equation for Henry's Law is:

C = k * P

Where:
C is the solubility of the gas in the liquid (in this case, nitrogen gas in water),
k is the Henry's Law constant for the specific gas and liquid at a given temperature,
P is the partial pressure of the gas above the liquid.

In this case, the Henry's Law constant (k) for N2 in water at 30 oC is given as 6.0 x 10-4 M/atm.

Now we can substitute the given values into the equation to calculate the solubility (C):

C = (6.0 x 10-4 M/atm) * (2.5 atm)

C = 1.5 x 10-3 M

Therefore, the solubility of nitrogen gas in water at a partial pressure of 2.5 atm is 1.5 x 10-3 M.