Final answer:
The gas sample with the highest pressure can be identified using a manometer, taking into account differences in mercury column height and whether the manometer is open or closed-end. Partial pressures contribute to the total pressure of a gas mixture.
Step-by-step explanation:
To identify the gas sample with the highest pressure, we must understand how a manometer works and how it relates to pressure measurements. At sea level, the atmospheric pressure is typically 760 mm Hg, or 1 atm, since these are standard reference values. For an open-end manometer, the pressure of the gas is the atmospheric pressure plus or minus the difference in height (h) of the mercury (Hg) column. If the mercury column is higher on the side open to the atmosphere, the gas pressure is lower than atmospheric pressure. If the mercury column is higher on the side connected to the gas, then the gas pressure is higher than atmospheric pressure.
In a closed-end manometer, there is no atmospheric pressure to consider on the closed side. The pressure of the gas is directly indicated by the height of the mercury column on the side open to the gas. The pressure in torr is equal to the height of the mercury column in mm.
Partial pressures refer to the pressures of individual gas components in a mixture. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each component gas.
When determining the boiling points of hydrocarbons C₂H6, C3H8, and C4H10, the molecular size and the intermolecular forces should be considered.