The solubility of oxygen in lakes high in the rocky mountains is affected by the altitude. if the solubility of o2 from the air is 2.67 ✕ 10-4 m at sea level and 25°c, what is the solubility of o2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? assume the temperature is 25°c, and that the mole fraction of o2 in air is 0.209 at both 12,000 ft and at sea level.

Explanation:

Henry's law states that the solubility of a gas is directly proportional to its partial pressure. The equation may be written as:

Where is Henry's law constant.

Our strategy will be to identify the Henry's law constant for oxygen given the initial conditions and then use it to find the solubility at different conditions.

Given initially:

Also, at sea level, we have an atmospheric pressure of:

Given mole fraction:

According to Dalton's law of partial pressures, the partial pressure of oxygen is equal to the product of its mole fraction and the total pressure:

Then the equation becomes:

Solve for :

Now we're given that at an altitude of 12,000 ft, the atmospheric pressure is now:

Apply Henry's law using the constant we found:

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

c. orbital shape i hope this is correct