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:

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.