Problem: Butane is a common fuel used in cigarette lighters and camping stoves. Normally supplied in metal containers under pressure, the fuel exists as a mixture of liquid and gas, so high temperatures may cause the container to explode. At 25.0°C, the vapor pressure of butane is 2.3 atm. What is the pressure in the container at 135°C (ΔH°vap = 24.3 kJ/mol)?

FREE Expert Solution

We can directly determine the vapor pressure of a certain molecule in a particular temperature using the Clausius-Clapeyron equation:

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Problem Details

Butane is a common fuel used in cigarette lighters and camping stoves. Normally supplied in metal containers under pressure, the fuel exists as a mixture of liquid and gas, so high temperatures may cause the container to explode. At 25.0°C, the vapor pressure of butane is 2.3 atm. What is the pressure in the container at 135°C (ΔH°vap = 24.3 kJ/mol)?

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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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Based on our data, we think this problem is relevant for Professor Aronskyy's class at BARUCH CUNY.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.