The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 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...
How many liters of the antifreeze ethylene glycol [CH2(OH)CH2(OH)] would you add to a car radiator containing 5.50 L of water if the coldest winter temperature in your area is −20.0°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.) What is the volume of antifreeze? L What is the boiling point of the solution?
Be sure to answer all parts. How many liters of the antifreeze ethylene glycol [CH2(OH)CH2(OH)] would you add to a car radiator containing 7.25 L of water if the coldest winter temperature in your area is -21.0°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.) What is the volume of antifreeze? L. What is the boiling point of the solution? oC
there's two questions :) Enter your answer in the provided box A solution is prepared by dissolving 396 g of sucrose (C12H2011) in 604 g of water. What is the vapor pressure of this solution at 30°C? (The vapor pressure of water is 31.8 mmHg at 30°C.) mmHg Be sure to answer all parts. How many liters of the antifreeze ethylene glycol (CH2(OH)CH (OH) would you add to a car radiator containing 5.75 L of water if the coldest winter...
How many liters of the antifreeze ethylene glycol [CH_2(OH)CH_2(OH)] would you add to a car radiator containing 6.50 L of water if the coldest winter temperature in your area is -13 degree C? (The density of ethylene glycol is 1.11 g/mL. Assume the density of water at -13 degree C is 1.00 g/mL.) L Calculate the boiling point of this water-ethylene glycol mixture. degree C
there's two questions :) Enter your answer in the provided box. The solubility of KNO3 is 155 g per 100.0 g of water at 75°C and 38.0 g at 25°C. What mass (in grams) of KNO3 will crystallize out of solution if exactly 275.0 g of its saturated solution at 75°C is cooled to 25°C The solubility of N, 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...
Please can you solve 1 &2 ASAP. Thank you. 1) Calculate the m olality of each of the following aqueous solutions: (a) 0.940 M KBr solution (density of solution 1.08 g/mL), (b) 29.2 percent by mass NaCl solution, (c) 14.3 g of sucrose (C12H20n) in 676 g of water. 2) The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is 5.6 x 104 mol/L. A deep-sea diver breathes compressed air with the partial...
Enter your answer in the provided box. The partial pressure of N2 in the air is 593 mm Hg at 1 atm. What is the partial pressure of N, in a bubble of air a scuba diver breathes when he is 132 ft below the surface of the water where the pressure is 5.00 atm? mm Hg
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?
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