🤓 Based on our data, we think this question is relevant for Professor Paredes' class at Clark College.

A sample of gas isolated from unrefined petroleum contains 90.0% CH_{4}, 8.9% C_{2}H_{6}, and 1.1% C_{3}H_{8} at a total pressure of 307.2 kPa. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)

We’re being asked to **calculate the partial pressures** of each component of a gas mixture composed of **90.0%** CH_{4}, **8.9%** C_{2}H_{6}, and **1.1%** C_{3}H_{8} with a total pressure of **307.2 kPa**.

Recall that the ** partial pressure of a gas (P_{Gas})** in a mixture is given by:

$\overline{){{\mathbf{P}}}_{{\mathbf{gas}}}{\mathbf{=}}{{\mathbf{\chi}}}_{{\mathbf{gas}}}{{\mathbf{P}}}_{{\mathbf{total}}}}$

where:

**χ**** _{Gas}** = mole fraction of the gas

**P _{total}** = total pressure of the gas mixture

Partial Pressure