Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 x 10-3 M/atm.

This answer worked better for me

P = P°*X

=> C = P°*X*k = 1.13atm * 0.21 * 1.3*10^-3M/atm = 3.085*10^-4M

3.085*10^-4M * 5L = 1.54*10^-3mol = 1.54mmol

1.54*MM(O2) = 1.54mmol * 32mg/mmol = 49.4mg

^

/ \
<(0o0)>
{ | | }
/ ( ) \
| |
^. ^

0O0

Well, let me put on my floating clown wig and calculate that for you!

First, we need to convert the pressure of air from atm to Molar concentration. We can use the ideal gas law, but let's keep it simple and use the mole fraction of oxygen given, which is 0.21.

So, the Molar concentration of oxygen in the bucket of water is 1.13 atm * 0.21 = 0.2373 atm.

Now, we can use Henry's law to calculate the mass of oxygen dissolved in water. Henry's law states that the concentration of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. The constant of proportionality (Henry's law constant) is given as 1.3 x 10-3 M/atm.

Therefore, the mass of oxygen dissolved in water is:

mass = concentration * volume
= (1.3 x 10-3 M/atm) * (0.2373 atm) * (5.00 L)
= 0.00153915 moles

Now, to convert moles to milligrams, we can use the molar mass of oxygen, which is approximately 32 g/mol.

mass = 0.00153915 moles * (32 g/mol) * (1000 mg/g)
≈ 49.2512 mg

So, the mass of oxygen dissolved in the 5.00 L bucket of water is approximately 49.2512 mg.

I hope that calculation made you giggle a bit!

To calculate the mass of oxygen dissolved in the water, we can use Henry's law, which states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

First, let's calculate the partial pressure of oxygen in the air. We can do this by multiplying the total pressure of air (1.13 atm) by the mole fraction of oxygen in air (0.21).

Partial pressure of oxygen = Total pressure of air x Mole fraction of oxygen in air
Partial pressure of oxygen = 1.13 atm x 0.21
Partial pressure of oxygen = 0.2373 atm

Next, we can use Henry's law to calculate the concentration of dissolved oxygen in water. Henry's law constant relates the concentration of a gas in a liquid to its partial pressure.

Concentration of oxygen in water = Henry's law constant x Partial pressure of oxygen
Concentration of oxygen in water = 1.3 x 10^(-3) M/atm x 0.2373 atm
Concentration of oxygen in water = 3.075 x 10^(-4) M

Now, let's convert the concentration of oxygen in water to mass using the molar mass of oxygen.

Molar mass of oxygen = 32 g/mol

Mass of oxygen dissolved in water = Concentration of oxygen in water x Volume of water

But the given volume of water is in liters, and we need to convert it to milliliters for the final answer.

Volume of water = 5.00 L = 5000 mL

Mass of oxygen dissolved in water = (Concentration of oxygen in water x Volume of water) x Molar mass of oxygen
Mass of oxygen dissolved in water = (3.075 x 10^(-4) M x 5000 mL) x 32 g/mol
Mass of oxygen dissolved in water = 49.2 mg

Therefore, the mass of oxygen dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 49.2 mg.

massO2=Hconstant*pressure*volume*molmass

= 1.3E-3*1.13*5L*32 grams=235mg\\check it.