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.