The partial pressure of O2 in your lungs varies from 25 mm Hg to 40 mm Hg. What mass of O2 can dissolve in 1.0L OF water at 25.0oC when the O2 partial pressure is 40. mm Hg?
p = kC
partial pressure = k*C (in molarity)
k = 769.2 L*atm/mol
Plug in 40 mm O2 (convert to atm first) and k and solve for C (in mols/L).
Convert to grams.
Well, I hope you're ready for some fun with gas solubility! Now, to calculate the mass of oxygen that can dissolve in water, you need to use Henry's Law. It states that the amount of a gas dissolved in a liquid is directly proportional to its partial pressure.
Now, let's get down to business. The solubility of oxygen in water is around 0.0013 mol/L per mm Hg at 25.0oC. So, if the partial pressure of oxygen is 40 mm Hg, you can multiply that by the solubility to find the molarity of oxygen in the water.
40 mm Hg * 0.0013 mol/L per mm Hg = 0.052 mol/L
Next, you need to multiply the molarity by the molar mass of oxygen to get the mass of oxygen that dissolves in 1.0L of water.
0.052 mol/L * 32 g/mol = 1.664 g
So, at a partial pressure of 40 mm Hg, approximately 1.664 grams of oxygen can dissolve in 1.0L of water at 25.0oC. Keep in mind that the solubility of oxygen will vary with different conditions. Oxygen may kiss water molecules differently in the future!
To calculate the mass of O2 that can dissolve in 1.0L of water at 25.0°C when the O2 partial pressure is 40 mm Hg, we can use Henry's law. Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
The equation for Henry's law is:
C = kP
Where:
C is the concentration of the dissolved gas in the liquid (in mol/L)
k is the Henry's law constant (specific for the gas and the liquid)
P is the partial pressure of the gas (in atm)
Since we're given the partial pressure in mm Hg, we need to convert it to atm:
1 atm = 760 mm Hg
Converting the given partial pressure to atm:
40 mm Hg * (1 atm / 760 mm Hg) = 0.0526 atm
Now, we need the Henry's law constant for O2 in water at 25.0°C. The value for k can vary, but typically for O2 in water it is around 0.0013 mol/L*atm.
Using the equation C = kP, we can rearrange it to solve for C:
C = kP
C = (0.0013 mol/L*atm) * 0.0526 atm
C = 0.00006838 mol/L
Now we need to convert the concentration in mol/L to mass in grams. The molecular weight of O2 is approximately 32.0 g/mol.
Converting the concentration to mass:
Mass = concentration * volume
Mass = (0.00006838 mol/L) * (1.0 L)
Mass = 0.00006838 mol * (32.0 g/mol)
Mass = 0.00219 g
Therefore, the mass of O2 that can dissolve in 1.0L of water at 25.0°C when the O2 partial pressure is 40 mm Hg is approximately 0.00219 grams.
To find the mass of oxygen that can dissolve in water at a given partial pressure, we can use Henry's Law. Henry's Law states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas.
The equation for Henry's law is:
C = k * P
Where:
C is the concentration of the gas in the liquid (in mol/L),
k is the Henry's Law constant,
P is the partial pressure of the gas (in mm Hg).
In this case, we want to find the mass of oxygen that can dissolve in 1.0L of water. To do this, we need to convert the concentration of the gas to mass using the molar mass of oxygen.
Let's break down the process step by step:
1. Convert the given partial pressure of oxygen to atm:
40 mm Hg = 40 / 760 atm (since 1 atm = 760 mm Hg)
P = 0.0526 atm
2. Determine the Henry's Law constant for oxygen in water at 25.0oC:
The value of k depends on the solute and solvent. For oxygen in water, the typical value is 0.0013 mol/L*atm.
3. Calculate the concentration of dissolved oxygen using Henry's Law:
C = k * P
C = 0.0013 mol/L*atm * 0.0526 atm
C = 6.838 × 10^-5 mol/L
4. Convert the concentration from mol/L to mass using the molar mass of oxygen:
Molar mass of oxygen (O2) = 32.0 g/mol
Mass = C * molar mass * volume
Mass = 6.838 × 10^-5 mol/L * 32.0 g/mol * 1.0 L
Mass = 0.00218896 g
Therefore, the mass of oxygen that can dissolve in 1.0L of water at 25.0oC when the O2 partial pressure is 40. mm Hg is approximately 0.00219 grams.