Final answer:
To find the ΔHvap, use the Clausius-Clapeyron equation. The ΔHvap is -38,160 J/mol. The normal boiling point is approximately 96 °C.
Step-by-step explanation:
Solution:
To find the ΔHvap, we can use the Clausius-Clapeyron equation:
ln(P₂/P₁) = (-ΔHvap/R)(1/T₂ - 1/T₁)
We can substitute the given values: P₁ = 92 torr, T₁ = 23 °C = 296 K, P₂ = 300 torr, and T₂ = 45 °C = 318 K. R is the ideal gas constant (0.0821 L·atm/mol·K).
Solving for ΔHvap, we get:
ΔHvap = (-8.314 J/mol·K)(ln(300/92))/(1/318 - 1/296))
ΔHvap = -38,160 J/mol
The normal boiling point is the temperature at which the vapor pressure equals atmospheric pressure at sea level. Since the atmospheric pressure is about 760 torr, we can use this pressure to find the normal boiling point.
Substituting the given values into the Clausius-Clapeyron equation and solving for T, we get:
T = (-8.314 J/mol·K)(ln(760/92))/(1/318 - 1/296))
T ~ 369 K ~ 96 °C