Final answer:
The boiling point of chloroform (CHCl3) can be calculated using the Gibbs free energy equation at the boiling point, where ΔG = 0. It simplifies to T = ΔHvap / ΔSvap, yielding approximately 333.7 K. Therefore, the closest option to the calculated boiling point is C) 330 K.
Step-by-step explanation:
To find the boiling point of chloroform (CHCl3) in kelvin, we need to use the given values for the enthalpy of vaporization (ΔHvap) and the entropy of vaporization (ΔSvap). The boiling point is the temperature at which the vapor pressure of the liquid equals the external pressure, commonly at 1 atm. We can use the thermodynamic equation that relates these quantities, which is the Gibbs free energy equation ΔG = ΔH - TΔS, where ΔG = 0 at the boiling point.
At the boiling point, ΔG = 0, thus the equation simplifies to 0 = ΔHvap - TΔSvap, from which we can solve for T,
T = ΔHvap / ΔSvap. Converting ΔSvap to kJ by dividing 87.5 J/(K⋅mol) by 1000 gives 0.0875 kJ/(K⋅mol). Plugging in the values ΔHvap = 29.2 kJ/mol and ΔSvap = 0.0875 kJ/(K⋅mol), we find that the boiling point of chloroform is approximately T = 29.2 kJ/mol / 0.0875 kJ/(K⋅mol), which results in a temperature of approximately 333.7 K. Thus, the closest option is C) 330 K.