Today in class Ms.K went over questions 2 a), b), and 4 (as shown below) from Solubility Equilibria Assignment #1. We were then told to complete and hand in questions 2 c) and d). Later on Ms.K told us we also had to finish questions 5, 6, 7, and 8 for tomorrow and she also added that our test on this unit will be on tuesday next week.
Next scribe is Megan.
Thursday, April 30, 2009
Wednesday, April 29, 2009
April 29, 2009
Hi~o(*∩_∩*)o~
......
The next scribe is... Ashley
^.^
In today's class, we proved the answers of question #3. b) c) d)
And then we went over the example 4 by Calculating Solubility Product in the white sheet..
And the example 5 by Determining Ion Concentrations from Ksp
......
The next scribe is... Ashley
^.^
Tuesday, April 28, 2009
Chemistry Chemical Equlibrium...
hello....
ahm,,, today in class Mrs. read over the first 3 pages of our new topic
1 page
2nd page
3rd page
Then after Mrs. K read those 3 pages we were assign to do no. 1 and 3 from the assignment sheet..
Here are the questions:
ans.
For question # 3 we only corrected letter a, so the rest of it are homework :D
ans.
I'm sorry if I can't post the test correction
but don't worry because it's in Mrs. K slide show :D
kkk... see yah all tomorrow...
next scribe is Yicong
good nyt 2 all of u :D
ahm,,, today in class Mrs. read over the first 3 pages of our new topic
1 page
2nd page
3rd page
Then after Mrs. K read those 3 pages we were assign to do no. 1 and 3 from the assignment sheet..
Here are the questions:
ans.
For question # 3 we only corrected letter a, so the rest of it are homework :D
ans.
I'm sorry if I can't post the test correction
but don't worry because it's in Mrs. K slide show :D
kkk... see yah all tomorrow...
next scribe is Yicong
good nyt 2 all of u :D
Sunday, April 26, 2009
Chemical Equilibrium
Hi! I'm your scribe for Thursday's class
I'm really sorry for the delay of this blog post, I totally forgot it but anyways I hope its not too late...here it is....
Ms. K went over the Chapter 18 Study guide..
Page1
Page2
page3
Page4
If the words in the scan isn't that clear just check Ms. K 's slide post... Tomorrow, Monday is our test... don't forget to review... Hope you all had a great long weekend... Good luck on our test tomorrow..^_^
Next scribe will be RaminaR18 ^_^....
Thursday, April 23, 2009
Wednesday, April 22, 2009
disrupting equilibrium systems
hello everyone!
ehh. this is Venice blogging today or tonight i guess for yesterday cause i missed it. 8-)
Yesterday we did a lab called disrupting equilibrium systems. the purpose of the lab was to let us observe for ourselves what Le Chatelier's principle means.
for those who dont know..
Chatelier's principle: if stress is applied to a system in a dynamic equilibrium, the system changes to relieve the stress.
so during this lab we made and mixed a bunch of solutions. we were to record our observations of colour for the before reactions and the colour for the after reactions.
YUPP.
and i cant think anymore. im to sleepy. late night rehearsals are killing me. is this good enough ms. k? roflolalalalala. ok goodnight.
ehh. this is Venice blogging today or tonight i guess for yesterday cause i missed it. 8-)
Yesterday we did a lab called disrupting equilibrium systems. the purpose of the lab was to let us observe for ourselves what Le Chatelier's principle means.
for those who dont know..
Chatelier's principle: if stress is applied to a system in a dynamic equilibrium, the system changes to relieve the stress.
so during this lab we made and mixed a bunch of solutions. we were to record our observations of colour for the before reactions and the colour for the after reactions.
YUPP.
and i cant think anymore. im to sleepy. late night rehearsals are killing me. is this good enough ms. k? roflolalalalala. ok goodnight.
April 22,2009
In today's class:
A.) Ms.K gave us 20 minutes or more to finish the questions from our Lab Sheet
B.) We went over the Questions 1-2 from Lesson 4 assignment (yellow sheets)
C.) Received Handouts
-Concentration versus time Graph
-Chapter 18 study guide (answer pages 1 to 3)
The following were the answers from Lesson 4 assignment:
1.For the reaction
PCl3(g) + Cl2(g) PCl5(g) ΔH = –92.5 kJ
predict the effect on the position of the equilibrium that results from
a) increasing the total pressure by decreasing volume. shift right
b) injecting more Cl2 gas without changing the volume. shift right
c) increasing the temperature. shift left (increasing the temperature tends to favour the endothermic reaction)
d) increasing the volume of the container. shift left
e) adding a catalyst. Adding a catalyst does not affect the equilibrium position
2.For the reaction
CH4(g) + H2O(g) + 49.3 kJ CO(g) + 3 H2(g)
predict the effect on the position of the equilibrium that results from
a) increasing temperature. shifts right (Increasing temperature favours the endothermic reaction)
b) decreasing temperature. shift to the left
c) decreasing the pressure.shifts equilibrium to the right
d) decreasing the volume of the container.shifting equilibrium to the left
e) adding a solid drying agent such as CaCl2 which reacts with H2O(g). shift towards the left
That's what we all did for today's class....
next scribe is Larlyn.....*_*
A.) Ms.K gave us 20 minutes or more to finish the questions from our Lab Sheet
B.) We went over the Questions 1-2 from Lesson 4 assignment (yellow sheets)
C.) Received Handouts
-Concentration versus time Graph
-Chapter 18 study guide (answer pages 1 to 3)
The following were the answers from Lesson 4 assignment:
1.For the reaction
PCl3(g) + Cl2(g) PCl5(g) ΔH = –92.5 kJ
predict the effect on the position of the equilibrium that results from
a) increasing the total pressure by decreasing volume. shift right
b) injecting more Cl2 gas without changing the volume. shift right
c) increasing the temperature. shift left (increasing the temperature tends to favour the endothermic reaction)
d) increasing the volume of the container. shift left
e) adding a catalyst. Adding a catalyst does not affect the equilibrium position
2.For the reaction
CH4(g) + H2O(g) + 49.3 kJ CO(g) + 3 H2(g)
predict the effect on the position of the equilibrium that results from
a) increasing temperature. shifts right (Increasing temperature favours the endothermic reaction)
b) decreasing temperature. shift to the left
c) decreasing the pressure.shifts equilibrium to the right
d) decreasing the volume of the container.shifting equilibrium to the left
e) adding a solid drying agent such as CaCl2 which reacts with H2O(g). shift towards the left
That's what we all did for today's class....
next scribe is Larlyn.....*_*
Saturday, April 18, 2009
Friday, April 17, 2008
Ms.Kozoriz wasn't in class that day, and so we had a sub, and it was Mrs.Karras(I think that was her). And she said we had to finished the lab, An Analogy for an Equilibrium Reaction, and also in the yellow worksheet that Ms.Kozoriz gave us, Lesson 3, we have to do questions 4-8 oAnd pretty much that happen in class. So my scribe is very short but yeah.
Next scribe is Albert
Next scribe is Albert
Thursday, April 16, 2009
Equilibrium Lab
Today's class was spent doing a lab. The sheet is called An Analogy for an Equilibrium Reaction. The purpose of the lab was to help familiarize us with a system in equilibrium and how certain conditions effect that system. We were allowed to share data but everyone must hand in their own lab.
The experiment:
First we had to transfer water from one cylinder to another by using straws then record the change in volume in each cylinder. This was repeated for three transfers until the data remained the same. Once this happened we had to had an additional 5ml to ONE of the cylinders (A) then repeated until we reached the point where three transfers gave the same data.
For the data a chart is required to record the number of transfers, volume of cylinder A, and volume of cylinder B. Next we had to plot the data on graph paper and answer the questions that followed. I'm not sure if the due date was set yet.
Tomorrow's scribe will be rawra=).
The experiment:
First we had to transfer water from one cylinder to another by using straws then record the change in volume in each cylinder. This was repeated for three transfers until the data remained the same. Once this happened we had to had an additional 5ml to ONE of the cylinders (A) then repeated until we reached the point where three transfers gave the same data.
For the data a chart is required to record the number of transfers, volume of cylinder A, and volume of cylinder B. Next we had to plot the data on graph paper and answer the questions that followed. I'm not sure if the due date was set yet.
Tomorrow's scribe will be rawra=).
Wednesday, April 15, 2009
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*
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*
Tuesday, April 14, 2009
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.
Wednesday, April 8, 2009
Monday, April 6, 2009
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
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
Sunday, April 5, 2009
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!!
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!!
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