Today was a day that was filled with lots of nitrogen, in all three of its forms (including the rare solid nitrogen which few people have ever seen)! We started with some note-taking which you can get off moodle(not posted yet). The notes dealt with a new formula that is called the ideal gas law.
R= PV/NT (couldn't paste equations onto blogger from word)
R is the gas constant. It is equivalent to .082057. P is pressure (atm), V is volume(L), N is the number of moles, and T is temperature (K). This equation certainly is ideal for us because it relates all the variables into one law and we only need 1 circumstance rather than 2. For example, the combined gas law requires 2 circumstances. That is why you need 2 V's (V1 and V2) and so on. The combined gas law is below and it should be used when you have 2 circumstances.
P1V1/T1=P2V2/T2
With these two equations you can solve ideal gas problems which is on the worksheet you received today in class. After much convincing and pestering from the boys in row 1, they were able to convince Liebs to do at least one demo today. So Liebs took some of that awesome liquid nitrogen that he dumped on the floor yesterday, and threw it into the vacuum chamber that the balloon was in yesterday. Liebs lowered the pressure so much that the liquid nitrogen began to boil and finally it became solid. Though its appearance looked foamy, you'd never be able to feel it because once the pressure began to return to 1 atm, it quickly began to revert back to its liquid form. Finally, he dumped it onto the floor where it turned into a gas. That's all 3 forms of nitrogen. Somebody, though I can't remember who, coined the phrase nitrogen party. It certainly was!
Tonight's homework is the prelab for the Molar Volume lab and to do the ideal gas problem worksheet. The next scribe will be Rachel M.
"Life is like a garden: Dig it" ~A wise Man that is not Joe R
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