Define the term equilibrium vapor pressure. Use a vapor-pressure table (check th

Question

Define the term equilibrium vapor pressure. Use a vapor-pressure table (check the Database link on the class web site) to look up and record below, the equilibrium vapor pressure of a sample of water at 85 degree C and at 68 degree C. Consider two closed containers each partially filled with liquid water one at 85 degree C and the other at 68 degree C. Can the pressure of water vapor in the gas phase in either container ever exceed the equilibrium vapor pressure at the particular temperature? Explain why or why not.

Explanation / Answer

Vapor pressure is the equilibrium pressure at which the rate of vaporization beomes equal to the rate of condensation at the given temperature. From the data tables, vapor pressure of water at 80 deg.c = 57.8150 Kpa and at 68 deg.c = 28.53 Kpa Whenever the pressure equals vapor pressure it is the saturation point and no further increase In pressure is possible since that is the equilibrium pressure.

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