The henry's law constant (kh) for o2 in water at 20°c is 1.28e-3 mol/l atm. how many grams of o2 will dissolve in 3.5 l of h2o that is in contact with pure o2 at 1.65 atm?

Answer : The mass of dissolved will be, 0.2365 grams

Explanation :

First we have to calculate the concentration of .

As we know that,

where,

= concentration of = ?

= partial pressure of = 1.65 atm

= Henry's law constant =

Now put all the given values in the above formula, we get:

The concentration of =

Now we have to calculate the moles of

Now we have to calculate the mass of

Therefore, the mass of dissolved will be, 0.2365 grams

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

first one is the correct answer