Final blog post

I learned so much this year.

 I started off the year knowing nothing about chemistry, feeling very overwhelmed because I had never taken physics either, so I decided to drop one of those classes. I dropped phyics and stuck with chemistry.(got back into physics later in the year).

I think I accomplished a lot this year. Got some pretty good marks after working hard and really trying to learn chemistry.

The chemistry teacher, Mrs.Cule, is probably the reason I stuck to chemistry. From day one, learning about electrons and protons she tried to help me understand it and eventually I did.  

I learned all kinds of things this year, like a whole bunch of things about gases - the ideal gas law and the general gas law, etc. I also learned about equilibrium, which was hard to understand at first but now I'm okay with it.

Little advice : It's easier to picture gas molecules and using common sense as to what would happen if you changed the size of the container or increased the concentration, you can think of the molecules as little kids in a room running around. More kids and less space = more collisions. It's easier than trying to remember word for word. (Learned this from Mrs.Cule also)

IA for Math - Solar System / End of the World

IA concept map

chem blog post for test

Le Chateliers Principle

I think that last little project we did on the haber process helped a lot. It kind of brought it all back, starting the project I really forgot all the rules of le chateliers principle but now I'm feeling more comfortable with it.


Concentration

Increasing concentration on reactants shifts the equilibrium to the product side (right).

Increasing concentration on products shifts the equilibrium to the reactants side (left).


Opposite with decreasing.


Temperature

exothermic reaction: An increase in temperature shifts the equilibrium to the reactants side.

endothermic reaction: An increase in temperature shifts the equilibrium to the products side. 


Opposite with a decrease in temperature.


Pressure

When you increase the pressure the equilibrium shifts to the side has the least # of moles of gas.

When you decrease the pressure the equilibruim shifts to the side that has the most # of moles of gas.

√2 sin 5 x -1 = 0

√2 sin 5 x = 1

sin 5x = 1/√2

5x = 3π/4 +- 2πn     or      5x = π/4 +- 2πn

x = 3π/20 +- 2πn/5, n E Z        x= π/20 +- 2πn/5 , n E Z

Haber Process video for chemistry

PIE... hah

This is so weird.... it actually works! Anybody know why???

Solving logarithmic equation Voicethread.
Had trouble with this one.... 
log5(x-1) +6 = log5 (2x+3)

hahah this is true... 

ZOEYYYYYYY