Textbook Problem

Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume):

$\text{ppmv of}X= \frac{\text{vol of}\text{Xat STP}}{\text{total vol of air at STP}} \times {10}^6$

On a certain November day, the concentration of carbon monoxide in the air in downtown Denver, Colorado, reached 3.0 × 10² ppmv. The atmospheric pressure at that time was 628 torr and the temperature was 0°C.

a. What was the partial pressure of CO?

b. What was the concentration of CO in molecules per cubic meter?

c. What was the concentration of CO in molecules per cubic centimeter?