Question

Acetic acid has a normal boiling point of 118∘C and a ΔHvap of 23.4 kJ/mol. What is the vapor pressure (in mmHg) of acetic acid at 35∘C?

Answer 1

To calculate the vapor pressure of acetic acid at 35°C, use the Clausius-Clapeyron equation. Convert temperatures to Kelvin and use the enthalpy of vaporization to solve for P2.

Step-by-step explanation:

To calculate the vapor pressure of acetic acid at 35°C, we can use the Clausius-Clapeyron equation, which relates the boiling point temperature, vapor pressure, and enthalpy of vaporization:

ln(P2/P1) = -(ΔHvap/R)((1/T2) - (1/T1))

First, we convert the temperatures to Kelvin: T1 = 118°C + 273.15 = 391.15 K, and T2 = 35°C + 273.15 = 308.15 K. We also convert the enthalpy of vaporization to J/mol: ΔHvap = 23.4 kJ/mol × 1000 = 23,400 J/mol.

Now we can plug these values into the equation to solve for ln(P2/P1). Rearranging the equation and solving for P2 gives us the vapor pressure of acetic acid at 35°C.