Question

Henry's Law Henry's Law states that the solubility of a gas in a liquid (at a constant temperature) is entirely dependent on the partial pressure of that gas above the liquid. Increasing the pressure of increases the presence of that gas in the solution. We have talked about soda, carbonated with CO). These sodas are carbonated by placing the soda under a high COpressure Considering Henry's Law for gas solubility, consider the top of Mt. Everest. The atmospheric pressure at the summit is much lower than at sea level, approximately 253 mmHg. a) If oxygen makes up 21% of the air, what is the partial pressure of oxygen gas at the summit? CO dissolved in soda CO), wubbles out of solution molecule 253 mmity & 211.02 02-53multas € 100 l Cola b) The partial pressure of oxygen in deoxygenated blood in the lungs is 100 mmHg. Given your calculation of Po, at the summit of Everest, is O more soluble or less soluble in blood than at sea level?

need help with part b please

Answer 1

A higher partial pressure of the gas to be dissolved means a higher solubility. Since the parttial pressure of 100 mmHg in the lungs is higher than that on everest (253 mmHg), O₂ cannot be dissolved at this pressure. Compare this to sea level where the pressure is around 760 mmHg, there is better dissolution