Answer :
Final answer:
The question asks to calculate the vapor pressure of ethanol at 55.7 °C using the Clausius-Clapeyron equation, given its vapor pressure at 63.5 °C and ethanol's enthalpy of vaporization.
Explanation:
The question revolves around using the Clausius-Clapeyron equation to calculate the vapor pressure of ethanol at a different temperature given the vapor pressure at a known temperature and the enthalpy of vaporization. We can rearrange the Clausius-Clapeyron equation into:
ln(P1/P2) = (∆Hvap/R)((1/T2) - (1/T1))
Where P1 and P2 are the vapor pressures at temperatures T1 and T2 respectively, ∆Hvap is the enthalpy of vaporization, and R is the gas constant. Given the known parameters, one can solve for the vapor pressure at 55.7 °C (328.85 K) using the vapor pressure at 63.5 °C as a starting point.
To solve the problem, you would first convert the given ∆Hvap from kJ/mol to J/mol (since R is given in J/K•mol), calculate the temperatures in Kelvin, then solve for P2 using the equation above.
