The lighter components are able to rise higher in the column before they are cooled to their condensing temperature, allowing them to be removed at slightly higher levels.
I hope this helps
Firstly we need to determine the partial pressure of O2:
We will now use the Henry's Law equation to determine the solubility of the gas:
Answer: Solubility is 2.7x10^-3 M
Density= mass/volume. volume= 12 x 6 x 10. 415/720=.57g/cm^3
Ok so, remember that t<span>he average atomic mass is what is seen on the periodic table. It is the average mass of all of the isotopes with their frequency taken into account. What you need to do is add the products of the masses and frequencies Just like this:</span>
<span>0.903*267.8 + 0.097*270.9
When you add it the result is what you are looking for</span>
