At a particular temperature, the solubility of He in water is 0.080 M when the partial pressure is 1.7 atm. What partial pressure of He would give a solubility of 0.510 M?
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3. At 20 °C, the solubility of oxygen gas in water is 1.38 × 10–3 M at a partial pressure of 1.0 atm. What is the solubility of O2 in water when its partial pressure is decreased to 0.21 atm at the same temperature?
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?
I need help with number 2 and 3 2. Given the following information, please find the partial pressure of He. Mole fraction T = 25.0°C V = 15.0L P = 1.30 atm 0.100 0.250 0.150 0.250 COM 3. At 20 °C, the solubility of oxygen gas in water is 1.38 x 10 Mat a partial pressure of 1.0 atm. What is the solubility of O, in water when its partial pressure is decreased to 0.21 atm at the same temperature?
The Henry's law constant at 25 °C for CO₂ in water is 0.035 M/atm. What would be solubility of CO₂, in molarity units, be in 1.0 L of water when the partial pressure of CO₂ is 3.1 atm?
The solubility of CO2 in water exposed to the atmosphere, where the partial pressure of CO2 is 3.87 10 atm, is 1.32 * 10 M. At the same temperature, what would be the solubility of pressurized CO2, at a pressure of 68 atm? a. 5.09 x 10*M b. 2.32 M C. 1920 M d. 4310 M How many mL of a 0.575 M glucose solution (MW=184 g/mol) would be needed to make 350 ml of a 0.320 M glucose solution?...
Show the calculations for both problems. 8) 575.9 g of AI(NO3)(molar mass = 212.996g/mol) was dissolved in 17.89 kg of water. What is the boiling point of this solution? Boiling point of pure water is 100.00 °C and the boiling point constant is 0.510 °C. A) 0.0771 °C (B) 100.077 °C C) 0.308 °C D) 100.308 °C E) 99.692 °C F) 99.923 °C 100=0.510 x. 1511 9) Calculate the solubility of carbon dioxide in water at 10.0 °C and a...
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...
Hi only want to know #2! I think the solubility would be the same. LABORATORY EXPERIMENTS IN GENERAL CHEMISTRY 370 GENERAL CHEMISTRY STUDY SHEET NO. 14 ) olagibh-elog.aob no 1. If 27 g of acetylene gas (C2H2) dissolves in 1.00 L of acetone at 1.0 atm, then what is the solubility of acetylene in acetone if the partial pressure of acetylene is increased to 12.0 atm? 2. In the above problem enough N, = 18.0 atm while that of acetylene...
the solubility of a gas in water is 0.010 g L-1 at 25.0 ºC with the partial pressure of the gas over the solution at 1.0 atm, predict the solubility of the gas at the same temperature but at triple the pressure.
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...