The Henry's law constant for nitrogen dissolved in water at 298 K is 8.68* 10⁹ Pa. Determine the mole fraction of nitrogen in water in equilibrium with air at a pressure of 1 atm and temperature of 298 K.

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Henry's law states that the partial pressure of a gas in equilibrium with a liquid is proportional to the mole fraction of the gas in the liquid. The Henry's law constant is the proportionality constant.The mole fraction of nitrogen in water can be calculated using the following equation:X_N2 = P_N2 / Hwhere:X_N2 is the mole fraction of nitrogen in waterP_N2 is the partial pressure of nitrogen in airH is the Henry's law constantThe partial pressure of nitrogen in air can be calculated using the following equation:P_N2 = y_N2 * Pwhere:y_N2 is the mole fraction of nitrogen in airP is the total pressure of airThe mole fraction of nitrogen in air is approximately 0.78. The total pressure of air is 1 atm. Therefore, the partial pressure of nitrogen in air is:P_N2 = 0.78 * 1 atm = 0.78 atmThe Henry's law constant for nitrogen dissolved in water at 298 K is 8.68 * 10^9 Pa. Therefore, the mole fraction of nitrogen in water in equilibrium with air at a pressure of 1 atm and temperature of 298 K is:X_N2 = 0.78 atm / (8.68 * 10^9 Pa) = 8.98 * 10^-10The mole fraction of nitrogen in water is approximately 8.98 ppm.

The Henry's Law Constant for Nitrogen Dissolved in Water at 298