🤓 Based on our data, we think this question is relevant for Professor Aronskyy's class at BARUCH CUNY.
We can directly determine the vapor pressure of a certain molecule in a particular temperature using the Clausius-Clapeyron equation:
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)?