Part 2: Clausius-Clapeyron Equation (Vapor pressure, temperature, and

\\\\Delta H

)\ Substances that vaporize easily are volatile (weaker IMF) and those that take more energy to vaporize are less volatile or nonvolatile (stronger IMF). Vapor pressure is related to the quantity of gas phase molecules above the surface of the liquid and is directly proportional to temperature. That is, at higher temperatures a larger proportion of molecules in the liquid phase may have enough energy to overcome IMF of the liquid and go into the gas phase (figure below). As such vapor pressure increases with temperature. In summary, vapor pressure depends upon temperature and strength of intermolecular forces.\ Figure 1: Kinetic energy aistribution of motecutes at rem temperuites\ For the following\ i. Rank in order from lowest to highest vapor pressure and justify your response.\ The Clausius-Clapeyron equation relates the enthalpy of vaporization to vapor pressure and temperature.\

ln((P_(2))/(P_(1)))=(\\\\Delta H_(rxn)\\\\deg )/(R)((1)/(T_(1))-(1)/(T_(2)))

\

R=8.3145(J)/(K*mol)

\ As such, you are able to determine the enthalpy of vaporization (

\\\\Delta H_(vap)\\\\deg

) of a liquid by measuring its vapor pressure at different temperatures. In this equation,

R

is the gas law constant in units of

(J)/(m)ol*K

. Be sure

\\\\Delta H

and

R

have the same units! We also assume that

\\\\Delta H_(vap)\\\\deg

is independent of temperature.\ 3

Part 2: Clausius-Clapeyron Equation (Vapor pressure, temperature, and H ) Substances that vaporize easily are volatile (weaker IMF) and those that take more energy to vaporize are less volatile or nonvolatile (stronger IMF). Vapor pressure is related to the quantity of gas phase molecules above the surface of the liquid and is directly proportional to temperature. That is, at higher temperatures a larger proportion of molecules in the liquid phase may have enough energy to overcome IMF of the liquid and go into the gas phase (figure below). As such vapor pressure increases with temperature. In summary, vapor pressure depends upon temperature and strength of intermolecular forces. Figure 1: Kinetic energy distribution of molecules at different temperatures 3) For the following i. Rank in order from lowest to highest vapor pressure and justify your response. ii. Identify which of these molecules is the most volatile. The Clausius-Clapeyron equation relates the enthalpy of vaporization to vapor pressure and temperature. ln(P1P2)=RHrxn(T11T21)R=8.3145KmolJ As such, you are able to determine the enthalpy of vaporization ( Hvap ) of a liquid by measuring its vapor pressure at different temperatures. In this equation, R is the gas law constant in units of J/molK. Be sure H and R have the same units! We also assume that Hvap is independent of temperature. 3