Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.21 given that k_H for O₂is 1.3 × 10^-3 M/ atm at this temperature. A) 49.4 mg B) 23.5 mg C) 9.87 mg D) 27.3 mg E) 13.7 mg

Question

Quizplus · Accepted Answer

To find the mass of oxygen dissolved, use Henry's Law: C = kH * P. Here, C is the concentration of dissolved oxygen, kH is the Henry's Law constant (1.3 × 10^-3 M/atm), and P is the partial pressure of oxygen (0.21 * 1.13 atm). Calculate C, then convert moles to mass using the molar mass of O2 (32 g/mol), and finally convert to mg for the total volume of 5.00 L.

Calculate the Mass of Oxygen (In Mg)dissolved in a 5