Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 M/atm.

Use Henry's Law to find the solubility of nitrogen in water. 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 formula is: $C=kP$, where $C$ is the solubility, $k$ is the Henry's law constant, and $P$ is the partial pressure of the gas.