# Problem: Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 C.What is the vapor pressure of ethanol at 15°C?

🤓 Based on our data, we think this question is relevant for Professor Ratliff's class at USF.

###### FREE Expert Solution

We’re being asked to determine the vapor pressure of ethanol at 15 ˚C, given the heat of vaporization and normal boiling point. For this problem, we can use the Clausius-Clapeyron Equation: where:

P1 = vapor pressure at T1

P2 = vapor pressure at T2

ΔHvap = heat of vaporization (in J/mol)

R = gas constant (8.314 J/mol•K)

T1 and T2 = temperature (in K). ###### Problem Details

Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 C.

What is the vapor pressure of ethanol at 15°C?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Clausius-Clapeyron Equation concept. You can view video lessons to learn Clausius-Clapeyron Equation. Or if you need more Clausius-Clapeyron Equation practice, you can also practice Clausius-Clapeyron Equation practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofEthanol has a heat of vaporization of 38.56 kJ/mol and a nor...as high difficulty.

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Our expert Chemistry tutor, Dasha took 7 minutes and 26 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.