The solubility of gas in a liquid is profoundly affected by pressure. this relation is expressed by henry's law, which states that the solubility of a gas in a liquid, expressed in moles per liter (or m), at a given temperature is directly proportional to the partial pressure of the gas over the solution. this relation can be expressed mathematically as solubility=k⋅p. the constant k is characteristic of the specific gas and p is the partial pressure of the gas over the solution usually expressed in atmospheres. the constant k usually has units of moles per liter per atmosphere and is reported at 25 ∘c. this expression can be used to calculate any of the three variables provided that the other two are known for any gas.1) air is a mixture of gases that is about 78.0% n2 by volume. when air is at standard pressure and 25.0 ∘c, then2 component will dissolve in water with a solubility of 4.88×10−4 m. what is the value of henry's law constant for n2 under these conditions? 2) the vapor pressure of benzene, c6h6, is 100.0 torr at 26.1 ∘c. assuming raoult’s law is obeyed, how many moles of a nonvolatile solute must be added to 100.0 ml of benzene to decrease its vapor pressure by 10.0% at 26.1 ∘c? the density of benzene is 0.8765 g/cm3.3) a 2.650×10−2m solution of nacl in water is at 20.0∘c. the sample was created by dissolving a sample of naclin water and then bringing the volume up to 1.000 l. it was determined that the volume of water needed to do this was 999.3 ml . the density of water at 20.0∘c is 0.9982 g/ml.