Questions: An old 0.500 L lecture bottle of triethylamine (N(CH2CH3)3) was found in a lab and needed for a synthesis reaction. A pressure regulator indicated a pressure of 33.0 psi, and the lab was at room temperature (25°C). What mass of vaporized triethylamine was left in the lecture bottle?
Transcript text: An old 0.500 L lecture bottle of triethylamine $\left.\left(\mathrm{N}_{(} \mathrm{CH}_{2} \mathrm{CH}_{3}\right)_{3}\right)$ was found in a lab and needed for a synthesis reaction. A pressure regulator indicated a pressure of 33.0 psi , and the lab was at room temperature $\left(25^{\circ} \mathrm{C}\right)$. What mass of vaporized triethylamine was left in the lecture bottle?
Solution
Solution Steps
Step 1: Convert Pressure to Appropriate Units
First, we need to convert the pressure from psi to atmospheres (atm) because the ideal gas law uses pressure in atm. The conversion factor is 1atm=14.696psi.
P=14.696psi/atm33.0psi=2.246atm
Step 2: Convert Temperature to Kelvin
The ideal gas law requires temperature in Kelvin. Convert the given temperature from Celsius to Kelvin.
T=25∘C+273.15=298.15K
Step 3: Use the Ideal Gas Law to Find Moles of Gas