Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and oxygen gas that should bubble out of 1.2 L of water upon warming from 25 "C to 50 C. Assume that the water is initially saturated with nitrogen and oxygen gas at 25 C and a total pressure of 1.0 atm. Assume that the gas bubbles out at a temperature of 50 ° C. The solubility of oxygen gas at 50 ° C' is 27.8 mg /L at an oxygen pressure of 1.00 atm. The solubility of nitrogen gas at 50 * C is 14.6 mg /L at a nitrogen pressure of 1.00 atm. Assume that the air above the water contains an oxygen partial pressure of 0.21 atm and a nitrogen partial pressure of 0.78 atm.

Express your answer using two significant figures.

 

The solubility of oxygen, O2, in water is 7.20 ✕ 10−4 mol/L at 0°C when the nitrogen pressure above water is 0.554 atm. Calculate the solubility of oxygen in water when the partial pressure of oxygen above water is 1.083 atm at 0°C? The Henry's Law constant for oxygen is 1.30 ✕ 10−3 mol/ L atm.

An air tank contains a mixture of nitrogen and oxygen at a total pressure of 4.30 atm. If the partial pressure of nitrogen is 0.92 atm, what is the partial pressure of oxygen in the tank?

a scuba diver breathes air (from a tank) which has a partial pressure for nitrogen of 4.0 atm. calculate the volume of nitrogen he must breathe out on his way to the surface based on the following: the atmospheric pressure is 1.0 atm; air is 78.1% nitrogen; the max solubility of nitrogen in blood under a partial pressure of nitrogen of 0.50 atm is 3.2 x 10-4 m; the total volume of the diver's blood is 5.0 l