Niwatori's Corner (Equilibrium Constant!)

O hayao gozaimasu

Niwatori-san with Chemistry once again round 2 but this time I'm elaborating my text in order to make the premise more understanding.

Bear with me if you don't understand.... (I'll do my best for ya guys and gals)

Currently in class we were learning about the Equilibrium Constant in the form of small K and big K. There are slight differences to the small K constant and the big K constant.

Well before I get into detail over the K constants there are a few definitions worth checking over
these consist of:

** Note that most of the info is in the handout Grade 12 CHEMISTRY : CHEMICAL EQUALIBRIUM the 1st page has Defining Equilibrium right below the title above.**

Dynamic Equilibrium - This is the state where the forward process is equal to the reverse process. The system is not actually stopping but always moving constantly showing a constant opposition.

Physical Equilibrium - A reversible physical process is where the rate of forward is equal to the rate of reverse.

**** Keep note the only time a reversible reaction can be in equalibrium is in a closed system**** "closed systems keep particles in and other particles to stay out. A form of consistency is shown between the particles eg. vapor vs condensation

****Equilibriums by the way look/seem unmoving but they actually are in motion****

Equilibrium law and Equilibrium Constant - Known as the Law of mass action/Equilibrium law by Cato Goldberg and Peter Waage in 1864. The Equilibrium law is suggested to be a ratio between the concentrations of the products to the reactants.
A value is then given from the ratios and this numerical value is the Equilibrium Constant

(Ok enough of the definitions now onto some real work! *raises sleeves up to shoulder length*)

****Keep note if Kc/Equalibrium constant what the value is equal to; this value determines either the reactants/products being favored in which
this is as follows: Kc = 1 reactants & products neither favored
Kc = more than 1; products concentration greater and is favored
Kc = less than 1; reactants concentration greater and is favored


I'll just head onto showing you how to get Equalibrium Concentrations since that part was from yesturday and it seems like we should note it
(Getting the Kc should be no problem but if you don't remember just ask around!)

We have info:
Set up an ICE table (ICE is abbriviated in to Intial concentration(I), Delta"change in" Concentrations(C) and equilibruim concentrations (E)

for example we are given 2 reactants with equal moles

I 2.00 2.00 0

C -x -x +2x

E 2 - x 2 - x 2x


Ill get into detail with this if you want later time is of an essense

Niwatori-san signing off--->

Next Scribe is miss Kayla! =D

*passes baton and then skoots away*

Equilibrium Problems 1

Equilibrium Problems1

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April 12 Blog

Seeing how Moffatt didn't blog, I'll take do it for him. We went through a little booklet called Grade 12 CHEMISTRY: CHEMICAL EQUILIBRIUM. (ASK MRS. KOZORIZ FOR THIS HANDOUT) We also had a booklet that has assignments. This booklet is called Equilibrium Project Assignment. We had to have question 1 done on the assignment. That is pretty much it.

Kinetics Review

Kineticsreview

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Monday April 6, 2009

Today's class began with Mrs.k presenting to us several potential energy diagram on the smart board. She then went over question from the handout that was given on Friday(Reaction rates). The answers will be uploaded by Mrs.k, so no worries. we were assigned to do question 4 and b(Factors affecting rate)

Some of us worked on chemical kinetics assignment # 1, which was due today. The assignment was handed out on Thursday, the same day the hypnotist show took place. For people that were present at the hypnotist show, i believe Mrs.k is giving you more time to work on it.

i guess that's it
next scribe is robel

Reaction Coordinate Diagrams

Rxnpotentialdiagrams

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SCRIBE

Hi guys.. its me Aldrin scribing for our laaaaaasst friday class, just before spring break.:(

First thing, I'm terribly sorry for doing this scribe soooo late. I'm sure i have a reason, hopefuly:).


Here is last Friday's Scribe!!

at the start of the class Mrs' K gave us two new handouts regarding "CHEMICAL KINETICS" .
She read us through it and we learned how to differentiate an EXOTHERMIC to an ENDOTHERMIC reaction. specially using a reaction coordinate diagram.

** In an Exothermic reaction, the products possess less energy than the reactants.
During the reaction, heat is lost from the system and [HEAT(delta H) is a negative value]



**In an Endothermic reaction, the products possess more potential energy than the reactants.
This energy is absorbed from the surroundings, increasing the systems energy content.
[HEAT(delta H) is a positive value]



we also learn about ACTIVATION ENERGY(EA) - minimum amount of energy required for colliding particles to produce a chemical reaction.

after that, we answer a couple of questions regarding it.

Kinetics Assignment #2 ( 1-3)


*just remember to label the diagram properly
*locate the activation energy
and the HEAT change - whether absorbed or release
*exothermic(change in heat is a negative value)
endothermic(change in heat is a positive value)

well thats all for my scribe..
again, i'm really sorry for a very late post.
Yonas to scribe for Monday.

see you guys tomorrow. have a good night everyone!!