When using the Claussius Clapeyron to solve for vapor pressure and calculating t

Question

When using the Claussius Clapeyron to solve for vapor pressure and calculating temp. I don't understand the steps. Can you break down each step? I'm confused when I should convert and where to use dividing or multiplying. Example: Ethanol has a heat vaporization of 38.6 kilojoules/ mol and a normal boiling point of 78C. 1. Find the K intercept 2. What is the vapor pressure at 15C
When using the Claussius Clapeyron to solve for vapor pressure and calculating temp. I don't understand the steps. Can you break down each step? I'm confused when I should convert and where to use dividing or multiplying. Example: Ethanol has a heat vaporization of 38.6 kilojoules/ mol and a normal boiling point of 78C. 1. Find the K intercept 2. What is the vapor pressure at 15C
Example: Ethanol has a heat vaporization of 38.6 kilojoules/ mol and a normal boiling point of 78C. 1. Find the K intercept 2. What is the vapor pressure at 15C

Explanation / Answer

Using the Clausius-Clapeyron equation.

ln(P2/P1)=(H/R)(1/T1-1/T2)

Here H is the heat of vaporization= 38.6 Kj= 38600 J

Here T1= 78 C = 78+273=351 K

T2= 15 C = 15+273= 288 K

ln(P2/760 torr)= 38600/8.314 (1/351-1/288)

ln(P2)-ln(760 torr)=4642.77(0.00063)

lnP2= -2.92 +lln 760

P2 = e^3.71

P2= 40.85 torr

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.