Gas Law Reflection

I have not prepared enough for the gas laws test, I understand Pv=nrt but I have not spent enough time doing practice problems or learning the applications of the laws. I should spend some time reviewing these before finals and making sure that i am confident finding partial pressure, molar mass, and the identity of a gas. I should spend more time viewing websites like these:

http://faculty.clintoncc.suny.edu/faculty/Mike.Lawliss/My_webpage/map/pvnrt.htm

http://www.westfield.ma.edu/cmasi/gen_chem1/Gases/ideal%20gas%20law/pvnrt.htm

http://ww2.chemistry.gatech.edu/class/peek/1310/notes/09-gases.pdf

http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/idegas.html

Gas Law Links

Here are some links that will help to learn gas laws. 

http://www.chemguide.co.uk/physical/kt/idealgases.html
http://www.engineeringtoolbox.com/ideal-gas-law-d_157.html
https://www.youtube.com/watch?v=BxUS1K7xu30

It is Important to understand the Algebra of Pv=nrt, as it can be rewritten in many different forms.
Most pproblems can be solved using this equation but one could be puzzled because they thought
you would always use the same form. So be prepared to use n=PV/rt or T=PV/nr.

   

Common Units

Here are some common units of pressure and the important temperature conversion we need to know:

 

Most often when using gas laws, you will need to get the temperature from degrees celsius to degrees kelvin. This is a VERY simple conversion that can be done by adding 273.15 to the degrees celsius reading as 0 degrees celsius is equivalent to 273.15 degrees kelvin. Here is an example:

26 degrees celsius+ 273.15 =299.15 Degrees Kelvin.

Gas Laws Intro

Now we are learning about the properties of gases. One can calculate the pressure a gas exerts, its temperature at a certain pressure, even it's unknown identity using the Ideal Gas Laws. Gases are interesting bits of matter as they are the only ones that can be compressed and have no definite volume. Here is the ideal gas law that we will use: Note* The Universal Constant is .0821

Phase Diagrams

Here are the phase diagrams that I need to know. 

 Notice that as a phase change is occuring the temperature remains dormant. Also notice that under the right conditions a solid can sublimate into a gas and a gas can deposite into a solid.

Energy In Reactions

Here's something weird: In an exothermic reaction, energy is released into the surroundings, making them very hot... in chemistry, we learn that this means that the chemical reaction is actually getting COLDER. Due to the release of energy (a net loss) the system is losing energy and heat therefore. The same is true of the opposite, endothermic. They make the surroundings cold by sucking out energy from surroundings, therefore gaining it and becoming WARMER.
https://www.khanacademy.org/test-prep/mcat/chemical-processes/thermochemistry/a/endothermic-vs-exothermic-reactions

Energy Intro

We've begun learning about energy and how it affects matter and that matter's states. A couple of thing happen when energy is given to matter. 1. It heats up. 2. The molecules that compose it move more quickly and bump into each other more. 3. A phase change can occur.