1 liter flask contains nitrogen along with a drop or two of water at 40° C, the total pressure being 760 Torr. If all the contents are transferred to another flask of 0.5L at the same temperature. The pressure of nitrogen setup in the second flask will be: (aqueous tension at 40 °C 55 torr):

Explanation

When a 1 liter flask containing nitrogen and a drop or two of water at 40°C is transferred to another flask of 0.5L at the same temperature, the pressure of nitrogen in the second flask can be calculated using Boyle's law. Boyle's law states that the pressure of a gas is inversely proportional to its volume at constant temperature. Initially, the total pressure in the 1 liter flask is 760 Torr. After transferring the contents to the 0.5L flask, the volume of the gas is halved. Therefore, according to Boyle's law, the pressure of nitrogen in the second flask will be twice the original pressure, which is: P2 = P1 * (V1 / V2) = 760 * (1 / 0.5) = 1520 Torr. However, we need to subtract the vapor pressure of water from this value to get the pressure of nitrogen alone. The vapor pressure of water at 40°C is 55 Torr. Therefore: P2 (dry gas) = P2 (wet gas) - aqueous tension = 1520 - 55 = 1465 Torr. Therefore, the pressure of nitrogen setup in the second flask will be 1465 Torr. Note: aq. Tension is independent of volume, and depends on temperature.