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?
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When the partial pressure of nitrogen is 2.65 atm, .981 N2 dissolves in 1.5 L of...
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
Question 12 0.75 pts What mass of nitrogen, N2(g), is in 981.00 L water when the partial pressure of nitrogen is 3.19 atm? kh for nitrogen in water is 0.00066 M/atm O 1.7 x 10-3 g O 2.1 x 10g O 5.8 x 101 g O 16 x 10 g 0 21g O 6.0 x 10-48
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.
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 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 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...
< > Question 15 The partial pressure of O2 and N2 gases are 0.252 atm and 0.125 atm. These gases are held in a 15.3L vessel at 88.3 °C. If the temperature and volume remain constant when 0.444 moles of argon are added, what will be the total pressure (atm)? atm Submit Question
8. The Henry's law constant for the solubility of nitrogen in water is 6.4 x 104 M/atm at 25°C. At 0.75 atm of N2, what mass of N2(8) dissolves in 1.0 L of water at 25°C? a. 4.8 x 104 g b. 8.5 x 104 g c. 4.5 x 10' g d. 1.3 x 104g e. 2.4 X X X 09 9 0
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.
}We mix 0.25 g of oxygen gas (O2) and 1.5 g nitrogen gas (N2) in a 2 L container at 20oC. Assuming both gases behave ideally, (a)what is the partial pressure of oxygen? (b)what is the partial pressure of nitrogen? (c)what is the total pressure in the container? Molar masses are 32 g/mol for oxygen and 28 g/mol for nitrogen.