What is the concentration of nitrogen in water when the partial pressure of nitrogen above the...
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
Calculate the concentration of CO2 in a soft drink that is bottled with a partial pressure of CO2 of 5 atm over the liquid at 25 °C. The Henry’s Law constant for CO2 in water at this temperature is 3.12 ´ 10–2 mol L–1 atm–1. 1. 0.16 2. 0.26 3. 1.26 4. 1.16 5. 0.56
Calculate the concentration of CO2 in water at 25°C when the pressure of CO2 over the solution is 6.1 atm. At 25°C, the Henry's law constant for CO2 in water is 3.1 × 10−2 mol/L · atm.
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?
1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm? 2.The carbon dioxide concentration in a bottle of club soda is 0.12 mol L-1 at 25 °C. What is the pressure of carbon dioxide in the headspace? The Henry’s Law constant for CO2 at...
1. What is the partial pressure of nitrogen in a container that contains 5.82 mol of oxygen, 7.90 mol of nitrogen, and 5.85 mol of carbon dioxide when the total pressure is 621 mmHg? A) 185 mmHg B) 186 mmHg C) 251 mmHg D) 420 mmHg E) 621 mmHg 2. Using the van der Waals equation, determine the pressure of 335.0 g of SO2(g) in a 5.70-L vessel at 661 K. For SO2(g), a = 6.865 L2 • atm/mol2 and...
Estimate the pH of an aqueous solution exposed to a partial pressure of ammonia (NH3) of 10-4 atm. Assume that the temperature is 25ºC, there are no other components in the water and that the Henry’s law constant for ammonia is 0.018 atm M-1. Cleary state any simplifying assumptions that you make.
the soluability of nitrogen gas at 35C and a nitrogen pressure of 0.756 atm is 10^-4 mol/L. what is the value of the henry's law constant in mol L^-1 atm ^-1?
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
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...