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:

**P _{1}** = vapor pressure at T

**P _{2}** = vapor pressure at T

**ΔH _{vap}** = heat of vaporization (in J/mol)

**R** = gas constant (8.314 J/mol•K)

**T _{1} and T_{2}** = temperature (in K).

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?

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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.

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Our tutors rated the difficulty of*Ethanol 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.

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