1.) Describe the two diagrams of a bottled carbonated beverage shown below as greater
pressure or lower pressure, and then as greater solubility or lower solubility. How do these two
examples illustrate the relationship between the solubility of a gas and its vapor pressure? Explain

2.) On the diagrams below, assume that each beaker contains an equal number of moles
of solute. Label each solution as concentrated or dilute. Then indicate the approximate
relative volumes of each solution by describing the surface level on each beaker.

If i refer to the bottle at the left hand side as A and the bottle at the right hand side as B. I can say that the bottle A contains solutes which are more soluble than the solutes in bottle B. consequently, A has a lower vapour pressure than B.

We can also see that the pressure in A is much higher than in B(as indicated by the length of the arrows). The higher the pressure, the greater the solubility of the gas. Henry's Law states that: The solubility of a gas in a liquid is directly proportional to the pressure of that gas above the surface of the solution.

Again let me call the beaker on the left A and the beaker on the right B. We can see that the beaker on the left contains 10 ml of solution while the beaker on the right contains 50 ml of solution. It follows that beaker A contains a more concentrated solution since that much amount of solute is contained in a smaller volume than in beaker B as shown in the image.