Given the data below,determine the normal boiling point of COCl₂. P₁ = 100 mmHg,t₁ = -35.6 °C,Δ_vapH = 27.4 kJ/mol A)278 °C B)-65.1 °C C)-36.4 °C D)5.0 °C E)-5.0 °C

Question

Quizplus · Accepted Answer

The normal boiling point of a substance is the temperature at which its vapor pressure equals 1 atm (760 mmHg). To find this, we can use the Clausius-Clapeyron equation, which relates the change in vapor pressure with temperature to the enthalpy of vaporization. Given the initial vapor pressure (100 mmHg) and temperature (-35.6 °C), along with the enthalpy of vaporization (27.4 kJ/mol), we can solve for the temperature at which the vapor pressure equals 760 mmHg. The correct answer, after performing the calculations, is 5.0 °C, indicating that the normal boiling point of the substance is 5.0 °C.

Given the Data Below,determine the Normal Boiling Point of COCl2

Given the Data Below,determine the Normal Boiling Point of COCl₂