Liquid ammonia boils at –33.4ºc and has a heat of vaporization of 23.5 kj/mol. what is its vapor pressure at –50.0ºc? (r = 8.314 j/k•mol)

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey

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