Lessons 15 and 16

Today we covered lesson 15 and lesson 16. Starting with lesson 15, the most important thing to understand is number density. Number Density is the number of gas particles per unit volume. It can be written in the equation density= n/V. Something that goes along with number density is gas pressure. The gas pressure increases as the number of gas molecules per unit of volume increases. P=k(n/V). Moreover, air pressure can be measured by determining the difference in height of the liquid. My homework may help explain all of that better!

In lesson 16, we first started with understanding a mole! A mole is a unit of measurement that chemists came up with in order to more easily measure gas particles. It is very difficult to measure each particle individually. Therefore, Avogadro's Law and the mole help simplify! One mole= 602,200,000,000,000,000,000,000 OR 6,022 times 10 to the 23. Going along with Avogadro's law, STP comes into play. It is the standard temperature and pressure (1atm and 273K). Equal volumes of gases contain equal numbers of gas particles if the temperature and pressure and the same (STP). Lastly! 1 mole= 22.4L at STP.

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