Final answer:
The solubility of a gaseous solute according to Henry's law is directly proportional to the partial pressure of the gas above the solution. Increasing the pressure of the gas to 760 torr from 152 torr at constant temperature will increase the solubility of the gas in the solution.
Step-by-step explanation:
The question concerns the solubility of a gaseous solute in water and how it changes with pressure according to Henry's law. When the pressure of a gas above a liquid is increased, Henry's law states that the solubility of the gas in the liquid will increase proportionally, provided the temperature remains constant. In the given scenario, a solution at 0°C and 152 torr absorbs a certain amount of the gaseous solute. To find out how the solubility changes when the pressure is increased to 760 torr, one would set up a direct proportion based on Henry's law:
S1 / P1 = S2 / P2
Where S1 is the initial solubility (1.45 × 10⁻³ g), P1 is the initial pressure (152 torr), S2 is the final solubility, and P2 is the final pressure (760 torr). By rearranging the equation and solving for S2, the new solubility under increased pressure at constant temperature can be calculated accurately.