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

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.