Problem: A certain substance has a heat of vaporization of 47.70 kJ/mol. At what kelvin temperature will the vapor pressure be 3.50 times higher than it was at 293K?

🤓 Based on our data, we think this question is relevant for Professor Addo-Mensah's class at TAMIU.

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FREE Expert Solution

We’re being asked to determine the temperature at which the vapor pressure is 3.50 times higher than it was at 293 K, given the heat of vaporization


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).


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Problem Details

A certain substance has a heat of vaporization of 47.70 kJ/mol. At what kelvin temperature will the vapor pressure be 3.50 times higher than it was at 293K?

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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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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Addo-Mensah's class at TAMIU.