Question

The Clausius-Clapeyron equation allows us to estimate the vapor pressure of a substance at any temperature. It also provides an easy way to estimate the heat of phase transition from the vapor pressures measured at two temperatures. Clausius - Clapeyron eq: $\ln\frac{P_1}{P_2} = \frac{\Delta H_{vap}}{R} (\frac{1}{T_2} - \frac{1}{T_1}) R = \frac{8.314 J}{mol K} P = pressure of any unit type because the term $\ln\frac{P_2}{P_1}$ is unit less T = temperature on the absolute scale ONLY $\Delta H_{vap}$ typically has units of kJ/mol and is called the enthalpy of vaporization 1) Vapor Pressure of Water Example: The vapor pressure of water is 1.00 atm at 373 K, and the enthalpy of vaporization is 40.7 kJ mol?¹. Estimate the vapor pressure at temperature 363 and 383 K respectively.

          The Clausius-Clapeyron equation allows us to estimate the vapor pressure of a substance at any temperature.
It also provides an easy way to estimate the heat of phase transition from the vapor pressures measured at two
temperatures.
Clausius - Clapeyron eq: $\ln\frac{P_1}{P_2} = \frac{\Delta H_{vap}}{R} (\frac{1}{T_2} - \frac{1}{T_1})
R = \frac{8.314 J}{mol K}
P = pressure of any unit type because the term $\ln\frac{P_2}{P_1}$ is unit less
T = temperature on the absolute scale ONLY
$\Delta H_{vap}$ typically has units of kJ/mol and is called the enthalpy of vaporization
1) Vapor Pressure of Water Example: The vapor pressure of water is 1.00 atm at 373 K, and the enthalpy of
vaporization is 40.7 kJ mol?¹. Estimate the vapor pressure at temperature 363 and 383 K respectively.

The Clausius-Clapeyron equation allows us to estimate the vapor pressure of a substance at any temperature.
It also provides an easy way to estimate the heat of phase transition from the vapor pressures measured at two
temperatures.
Clausius - Clapeyron eq: ln(P1)/(P2) = (Δ Hvap)/(R) ((1)/(T2) - (1)/(T1))
R = (8.314 J)/(mol K)
P = pressure of any unit type because the termln(P2)/(P1)is unit less
T = temperature on the absolute scale ONLYΔHvaptypically has units of kJ/mol and is called the enthalpy of vaporization
1) Vapor Pressure of Water Example: The vapor pressure of water is 1.00 atm at 373 K, and the enthalpy of
vaporization is 40.7 kJ mol?¹. Estimate the vapor pressure at temperature 363 and 383 K respectively.

Added by Joy C.

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