2. Use the ideal gas law to relate mixing ratios (ppm, percent, etc.) to partial pressures, mass densities (e.g. mg/m?) or number densities (e.g. molecules per cm) for individual traces gases. A. For instance, what was the partial pressure of CO on February 7 when it reached 416.5 ppm at Mauna Loa, Hawaii? (Assume 677 mbar pressure and 3 C ambient temperature.) link: Global Monitoring Laboratory Carbon Cycle Greenhouse Gases (0030.go), B. What was the cogmass density in mg/m3? (Recall: PV-nRT: R-8,314 m? Pa K-1 mol-1: 1 bar = 105 Pa; CO2 molar mass 44.01 g/mol) C. If the humidity at that time was 13.9% RH, what does that mean? D. Finally, what was the mixing ratio (in %) of water in the atmosphere at that time? (You'll need to know that the saturation vapor pressure of water at 3 C is 7.6 mbar) links: ESRI Global Monitoring Division Mauna Loa Observatory.noaa.gov) e Dew Point and Relative Humidity Calculations (noaa.gov). Water Saturation Pressure (engineeringtoolbox.com)