The solubility of CO in water at 0°C and 1 atm CO pressure is 0.0354 mg of CO in 1 mL of water. Calculate the
molarity of aqueous CO solution at the normal partial pressure of CO of 0.00036 atm?
A)3.2×10-3M
B)2.9×10-4M
C)1.6×10-3M
D)1.3×10-5M
E)4.5×10-7M
The solubility of CO in water at 0°C and 1 atm CO pressure is 0.0354 mg...
Knowing that at 0 oC and an oxygen pressure of 1.00 atm, the aqueous solubility of O2 (g) is 48.9 mL O2 per liter. The approximate values for the molarity of O2 (g) in solution and the partial pressure of O2 above a 8.23 x 10-4 M O2 (g) saturated aqueous solution at 0 oC are respectively: A. 2.18 M and 3.78 x 10-4 atm B. 2.18 x 10-3 M and 0.378 atm C. 0.0446 M and 0.0179 atm D....
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?
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...
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...
Use Henry's law to determine the molar solubility of helium at a pressure of 1.3 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. I am having trouble figuring out the partical pressure of He is. I know that I use this equation: s=kp
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?
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?...
The solubility of CO gas in water is 0.158/(100 mL) at a CO, pressure of 760 mmHg Review You may want to reference Pages 259-262) Section 3.4 while completing this problem Part A What is the solubility of CO, in a soft drink (which is mainly water) that was borted under a CO, pressure of 4.1 atm? Express your answer using two significant figures. Part A Mass of glucose needed to prepare 305.0 mL of 24 % w/v glucose (C...
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...
The solubility of CO2 in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility at a partial pressure in air of 0.00049 atm? Assume that CO2 obeys Henry's law.