This question involves Henry's Law, which relates the solubility of a gas in a liquid to the partial pressure of the gas above the liquid. Henry's Law is expressed as:

$P=K_H\times x$

where $P$ is the partial pressure of the gas, $K_H$ is Henry's law constant, and $x$ is the mole fraction of the gas in the solution.

Rearranging for solubility (x):

$x=\frac{P}{K_H}$

This shows that solubility is inversely proportional to Henry's constant for a given pressure. A lower $K_H$ means higher solubility.

Given Henry's constants: w (0.5 kbar), x (2 kbar), y (35 kbar), z (40 kbar). Since solubility decreases as $K_H$ increases, the order of solubility is: w > x > y > z.

In the plots, solubility (x-axis) should increase from left to right. The correct plot must show the line for gas w (lowest $K_H$, highest solubility) having the steepest slope, and gas z (highest KH, lowest solubility) having the least steep slope, because slope is proportional to $K_H$ (from $P=K_H\times x$).

Thus, the correct plot is the one where the lines are in order of increasing slope from left to right: w (least slope), then x, then y, then z (steepest slope). This corresponds to the second option.

Related Topics

Henry's Law: Describes the solubility of gases in liquids. It states that the amount of gas dissolved is proportional to its partial pressure, with the constant $K_H$ being specific to each gas-solvent pair at a given temperature. Lower $K_H$ indicates higher solubility.

Solubility of Gases: Affected by pressure (Henry's Law), temperature (solubility decreases with temperature for most gases), and nature of gas and solvent.

Formulae

Henry's Law: $P=K_H\times x$

Solubility: $x=\frac{P}{K_H}$