The ΔHvap of a certain compound is 34.68 kJ·mol–1 and its ΔSvap is 93.60 J·mol–1·K–1. What it the boiling point of this compound?
I worked this elsewhere.
To determine the boiling point of a compound, we need to use the equation:
ΔG = ΔH - TΔS
where ΔG is the change in Gibbs free energy, ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature in Kelvin.
At the boiling point, the Gibbs free energy change (ΔG) is zero, so we can rearrange the equation to solve for T:
0 = ΔH - TΔS
Rearranging the equation:
TΔS = ΔH
T = ΔH / ΔS
Now, let's plug in the values given in the problem:
ΔH = 34.68 kJ·mol–1 = 34.68 × 10^3 J·mol–1
ΔS = 93.60 J·mol–1·K–1
T = (34.68 × 10^3 J·mol–1) / (93.60 J·mol–1·K–1)
T = 371.79 K
Therefore, the boiling point of this compound is approximately 371.79 Kelvin.