4. The solubility of nitrogen gas in water at 25°C and a partial pressure of N2 of 0.78 atm is 5.5×10–4 mol/L.
A. Calculate kH, Henry’s Law constant for nitrogen gas, at this temperature using the solubility at 0.78 atm. S = kH × P
4. The solubility of nitrogen gas in water at 25°C and a partial pressure of N2...
4. The partial pressure of nitrogen in air is 0.78 atm at 25 °C on a clear day, and the solubility of N2 in water is 5.3 × 10–4 M. What is the partial pressure of N2 when its solubility in water is 1.1 × 10–3 M at the same temperature?
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.
Henry’s law states that the solubility of a gas is directly proportional to the partial pressure of the gas if the temperature is constant. Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the Henry’s Law Constant (kH) for N2, O2, and CO2 in the textbook. a) Calculate the solubility (concentration in...
What partial pressure of N2 gas (in mm Hg) is required to maintain a solubility of 4.17×10-3 g/L in water at 25 °C? kH for N2 at 25 °C is 6.47×10-4 mol/L·atm.
What is the concentration of nitrogen in water when the partial pressure of nitrogen above the solution is 0.826 atm. Henry’s law constant for this system is 6.8x10^-4 mol/L atm.
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is 5.6 × 10-4 mol/L A deep- sea diver breathes compressed air with the partial pressure of N2 equal to 4.3 atm. Assume that the total volume of blood in the body is 5.4 L. Calculate the amount of N2 gas released (in liters at 37°C and 1.00 atm) when the diver returns to the surface of the water, where the partial pressure of...
need #7-10 answered 6. The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 x 10 mol/L. What is the value of the Henry's Law constant in mol/L-atm? A) 6.8 × 10-4 mol/L-atm B) 4.7 x 10 mol/L-atm C) 3.2 × 104 moVL-atm D) 9.0 x 10 mol/L atm E) 1.5 x 10mol/L atm 7. According to Raoult's law, which statement is false? A) The vapor pressure of a solvent over a solution decreases...
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is 5.6 x 10 mol/L. A deep- sea diver breathes compressed air with the partial pressure of N2 equal to 3.6 atm. Assume that the total volume of blood in the body is 4.7 L. Calculate the amount of N2 gas released (in liters at 37°C and 1.00 atm) when the diver returns to the surface of the water, where the partial pressure of...
When the partial pressure of nitrogen is 2.65 atm, .981 N2 dissolves in 1.5 L of water. What is the Henry"s constant, Kh, for nitrogen?
what partial pressure of He gas (in mm Hg) is required to maintain a solubility of 3.43x10^-4 g/L in water at 25 degrees C? kH for He at 25 degrees C is 3.26x10^-4 mol/L•atm. _________mm Hg