Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and oxygen gas that should bubble out of 1.8 of water upon warming from 25degree C to 50degree C . Assume that the water is initially saturated with nitrogen and oxygen gas at 25degree C and a total pressure of 1.0atm . Assume that the gas bubbles out at a temperature of 50degree C . The solubility of oxygen gas at 50degree C is 27.8mg/L at an oxygen pressure of 1.00atm . The solubility of nitrogen gas at 50 is 14.6mg/L at a nitrogen pressure of 1.00atm . Assume that the air above the water contains an oxygen partial pressure of 0.21atm and a nitrogen partial pressure of 0.78atm .
Use 2(3x - 7) + 4 (3 x + 2) = 6 (5 x + 9 ) + 3 to solve
will the answer be 5.25L??
To solve this problem, we will use Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.
First, let's calculate the mole fraction of nitrogen and oxygen gas in the air above the water at 50°C. The mole fraction is calculated by dividing the partial pressure of each gas by the total pressure.
For nitrogen gas:
Mole fraction of nitrogen gas = nitrogen partial pressure / total pressure
Mole fraction of nitrogen gas = 0.78atm / 1.0atm
Mole fraction of nitrogen gas = 0.78
For oxygen gas:
Mole fraction of oxygen gas = oxygen partial pressure / total pressure
Mole fraction of oxygen gas = 0.21atm / 1.0atm
Mole fraction of oxygen gas = 0.21
Next, we'll use the solubilities of nitrogen and oxygen gas at 50°C to calculate the amount of each gas that can dissolve in 1.8L of water.
For nitrogen gas:
Solubility of nitrogen gas = 14.6mg/L
Amount of nitrogen gas dissolved = solubility of nitrogen gas * volume of water
Amount of nitrogen gas dissolved = 14.6mg/L * 1.8L
Amount of nitrogen gas dissolved = 26.28mg
For oxygen gas:
Solubility of oxygen gas = 27.8mg/L
Amount of oxygen gas dissolved = solubility of oxygen gas * volume of water
Amount of oxygen gas dissolved = 27.8mg/L * 1.8L
Amount of oxygen gas dissolved = 50.04mg
Now, we can calculate the amount of nitrogen and oxygen gas that will bubble out of the water when it is warmed from 25°C to 50°C. Since the solubility values were given at 1.0atm pressure, we'll assume that the partial pressure of nitrogen and oxygen gas at 50°C is also 1.0atm.
For nitrogen gas:
Amount of nitrogen gas that bubbles out = Amount of nitrogen gas dissolved at 25°C - Amount of nitrogen gas dissolved at 50°C
Amount of nitrogen gas that bubbles out = 26.28mg - 1.8L * nitrogen solubility at 50°C
Amount of nitrogen gas that bubbles out = 26.28mg - 1.8L * 14.6mg/L
Amount of nitrogen gas that bubbles out = 26.28mg - 26.28mg
Amount of nitrogen gas that bubbles out = 0mg
For oxygen gas:
Amount of oxygen gas that bubbles out = Amount of oxygen gas dissolved at 25°C - Amount of oxygen gas dissolved at 50°C
Amount of oxygen gas that bubbles out = 50.04mg - 1.8L * oxygen solubility at 50°C
Amount of oxygen gas that bubbles out = 50.04mg - 1.8L * 27.8mg/L
Amount of oxygen gas that bubbles out = 50.04mg - 50.04mg
Amount of oxygen gas that bubbles out = 0mg
Therefore, the total volume of nitrogen and oxygen gas that should bubble out of the water when warmed from 25°C to 50°C is 0L.