HollyAsChemBlog: May 2016

Quiz Prep

Before the quiz on Friday, I found many websites for practice to differentiate between the three laws and to be more familiar with the concepts of gases. Here are some links I used to prepare for my quiz:
http://ed.ted.com/lessons/1207-1-a-bennet-brianh264

http://www.sparknotes.com/chemistry/gases/ideal/section2.rhtml

http://www.proprofs.com/quiz-school/story.php?title=gas-laws-review-quiz-20-items

http://www.sciencegeek.net/Chemistry/taters/Unit7GasLaws.htm

http://antranik.org/wp-content/uploads/2011/11/charles-boyle-avogadro-law-combined-gas-law.jpg

The last lesson we had before the quiz was introducing us to Avogadro's Law. This law states that for a gas at constant temperature and pressure, the volume is directly proportional to the number of moles present, which means that the formula looks like this:

http://thescienceclassroom.org/wp-content/uploads/2013/04/Avogadros-Law.png

We had to also use our mole road map for the volume and mass of what we were dealing wit. One important number for STP we had to memorize was 22.4L.
Here is how it would look:

https://elearning.kctcs.edu/bbcswebdav/users/kmuller0001/SoftChalk%20Files/CHE%20120%20Chapter%205/Vn.jpg

Also, the graph would remain linear:

https://s3.amazonaws.com/classconnection/186/flashcards/5446186/gif/graph-avogadro-1514FE9BE407D213356.gif

Practice for this law:
http://www.chemteam.info/GasLaw/Gas-Avogadro.html
http://dvhsgaslaws.weebly.com/avogadros-law.html

Charle's Law

The second day in lessons, we added to our gas laws and learned Charle's Law. This states that temperature and volume vary directly with each other, using the same formula, and this is at constant pressure. It is important to remember that this also must be done in Kelvin, so to convert from celsius to Kelvin, you have to add 273.15 to the original C.
This is what the formula is directly for this, and what it would look like:

https://upload.wikimedia.org/math/9/6/8/9682f75ffd644c1e723156ad5919c8a6.png

http://wps.prenhall.com/wps/media/objects/4678/4790892/images/aabjvhoa.jpg

The graph of this relationship would also look like this:

http://chemwiki.ucdavis.edu/@api/deki/files/8688/=CharlesLaw_(2).jpg?revision=1

Here are more links for practice:
http://www.chemteam.info/GasLaw/WS-Charles.html
http://science.widener.edu/svb/tutorial/charleslawcsn7.html

Gas Laws Intro

Our first lesson in this unit introduced us into the characteristics of gases and measuring pressures. We learned that ages expand spontaneously to fill their container, have no definite volume, are highly compressible, form homogeneous mixtures, and have molecules that are relatively far apart from one another.
Then, we went into converting into different units of pressure, where we had to memorize a similar chart:

https://i.ytimg.com/vi/mQn1Lat73AE/maxresdefault.jpg

Then, we learned about Boyle's law, which come of the basis of:

http://patentimages.storage.googleapis.com/EP0023910B1/imgb0016.png

This law states that relationship between pressure and volume is an inverse relationship, and holds true at constant temperature and moles. We then did some practice problems and looked at how the law works.

https://d2gne97vdumgn3.cloudfront.net/api/file/jMkrpsxQ5epbGnRIvowW

Here are some links to help with this lesson and overall gasses:

http://www.chemteam.info/GasLaw/WS-Boyle.html

https://www.youtube.com/watch?v=ZoGtVVu3ymQ

Second Phase Lesson

The second lesson had much more information than the first, and was pack with memorizing graphs and flow charts.
To start, we went through the flow chart to determine what kind of inter and intramolecular forces were within a compound.
This is the flow chart that we followed, and we went over being polar and how hydrogen bonding examples needed to make FONCLs (phone calls).

http://schoolbag.info/chemistry/central/central.files/image1460.jpg

We then went to look at examples that determined what state a compound was in, thus making us determine if the intramolecular force was covalent or ionic, and what the intermolecular force was based on the flow chart.
Next we looked at various curves so we could see the differences in phase changes. This is similar to what ours looked like.

https://writer.zoho.com/image.do?imgurl=43f284c1e0ba6646e2d2a98b8a52495191ec6d7cf7d22a0458f6d938d98b4eb1a7800cecd6ac3d9ca48373fdd0cecca6

We then looked at phase diagrams and did situations to where the compound would be.

http://www.kentchemistry.com/images/links/matter/Phase.gif

Here are some extra links for practice:
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch14/phase.php
http://www.sciencegeek.net/APchemistry/APtaters/PhaseDiagrams.htm
https://www.khanacademy.org/test-prep/mcat/chemical-processes/covalent-bonds/a/intramolecular-and-intermolecular-forces

New Energy Phase Unit

Lately in Chemistry, we have gone over the Unit of phase changes where we have gone through the bonding forces as well as the physical properties between the different phases. First we went over the differences in energies, where kinetic is in motion. Also, and important thing to remember was energy lost=energy gained.
Next we learned about end and exothermic processes.
Here is a picture demonstrating how endothermic take in energy and exothermic release energy

https://dr282zn36sxxg.cloudfront.net/datastreams/f-d%3Adf0a2687d885c997ec852a60b09181c51b0a234ada9136e0288d4e8c%2BIMAGE_THUMB_POSTCARD%2BIMAGE_THUMB_POSTCARD.1

The last big part of this lesson was the formula Q=Mc(Tf-Ti)
to plug into this formula, you must know that Q is heat in joules, m is mass in grams, c is specific heat in (J/g C), and T is change in temp.
This shows the process: