Final answer:
To estimate the enthalpy of vaporization for ethanol, we use the Clausius-Clapeyron equation with the provided vapor pressures at 20.0 °C and 63.5 °C. By solving the equation, we can find the energy required for ethanol to transition from liquid to vapor.
Step-by-step explanation:
The vapor pressure of a liquid at a certain temperature is the pressure exerted by its vapor when the liquid and vapor are in dynamic equilibrium. To estimate the enthalpy of vaporization for ethanol, we can use the Clausius-Clapeyron equation, which relates the change in vapor pressure with temperature to the heat required to vaporize the liquid.
Using the information that at 20.0 °C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53.3 kPa, we apply the Clausius-Clapeyron equation:
ln(P2/P1) = -(\Delta H_{vap})/R · (1/T2 - 1/T1)
Where P1 and P2 are the vapor pressures at temperatures T1 (293.15 K) and T2 (336.65 K) respectively, R is the gas constant, and \(\Delta H_{vap}\) is the enthalpy of vaporization. By rearranging and solving for \(\Delta H_{vap}\), we can estimate its value.