Determine the atmospheric pressure and calculate the solubility of oxygen in the lake in the Rocky Mountains. The Henry's law constant at 5°C is 1.6 x10-3 mol/lit atm. The total atmospheric pressure in Denver is 0.66 atm. The abundance of O2 remains constant at 20.95%.
Mole fraction of O2 = Volume fraction = %O2 in air / 100 = 0.2095
From Henry's law, we have the relation:
PO2 = mole fractionn of O2 * Atmospheric pressure = 0.2095 * 0.66 = 0.1383 atm
Solubility = KH * PO2 = 1.6 * 10-3 * 0.1383 = 2.213 * 10-4 mol/liter
Determine the atmospheric pressure and calculate the solubility of oxygen in the lake in the Rocky...
Calculate the solubility of oxygen in water at a partial pressure of O2 of 343 torr at 25°C. The Henry's Law constant for oxygen in water is 1.28 x 10 mol/(atm L). mol/L
1.The solubility of O2 in water is 0.590 g/L at an oxygen pressure of around 15.5 atm. What is the Henry's law constant for O2 (in units of mol/L
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.
The solubility of oxygen gas at 35.1 °C and a oxygen pressure of 649 mmHg is 8.06 × 10−3 g/L. What is the Henry's Law constant in mol⋅L−1⋅atm−1?
The partial pressure of O2 in air at sea level is 0.21 atm. The solubility of O2 in water at 20 ∘C , at 1 atm gas pressure, is 1.38×10−3 M. Using Henry's law and the data in the introduction, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 ∘C and an atmospheric pressure of 660 torr .
Lake Titicaca is situated at an altitude of 3810 m in the Bolivian Andes. Calculate the solubility of oxygen (in mg/L) in this lake at a temperature of 8.47 ºC. The Henry's Law constant at this temperature is 1.90×10-8 mol L-1Pa-1
Use Henry's law to determine the molar solubility of helium at a pressure of 1.1 atm and 25 degree C. Henry's law constant for helium gas in water at 25 degree C is 3.70-10^-4 M/atm. You can treat Henry's law constant as an equilibrium constant. The goal of this problem is to find the concentration of helium dissolved in water that would be in equilibrium with the helium pressure over the water of 1.1 atm according to K = [He/P_He].
5. The solubility of CO2 in water at 25 °C and 1 atm is 0.034 mol/L, W CO2 in carbonated water, if CO2 has a partial pressure of 0.0003s solubility ot atmospheric conditions? (5 points) atm under normal 6. The atmosphere contains 0.93 mol% argon, what is the partial pressure of argon at normal conditions of 1 atm and 25 °C? If the solubility of argon in water is 0.0150 mo/L under normal atmospheric conditions, what is Henry's Law Constant...
how could you detect the presence of At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1,00 atm? Number At 298 K, what is the solubility of oxygen in water exposed to air at 0.893 atm? Number If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from...
At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 0.892 atm? If atmospheric pressure suddenly changes from 1.00 atm to 0.892 atm at 298 K, how much oxygen will be released from 4.60 L of water in an unsealed container?