On Thursday we went over and corrected the Equilibrium Project Assignment, pages 1 questions 1-4 and page 2 questions 5-11. After that we worked on Lesson 3 Homework Assignment and did questions 1-5.
We also were given a assignment that is to be handed in Determining Equilibrium.
On Friday we did our Equilibrium & Le Chatelier Analogy Lab which should be handed in today.
That wraps up what we did before the weekend.
Monday, April 26, 2010
Wednesday, April 14, 2010
Wednesday, April 14
We went over yesterday homework (page 32, 33 and part B on page 34). We have to do Kinetics assignment #4 to hand in on Friday.
Tomorrow, we'll go straight to Ms. Truong's room at the beginning of class.
Test is on Friday on Chemical Kinetics. Study!!
Erick is to scribe next
Tomorrow, we'll go straight to Ms. Truong's room at the beginning of class.
Test is on Friday on Chemical Kinetics. Study!!
Erick is to scribe next
Tuesday, April 13, 2010
Rate Law
Helloooooooooooo everyone,
Today we learned about rate law, reaction order, and calculating rate order. We did example 2 on page 28 in the blue booklet. For homework, we have to do page 32, 33, and part B on page 34.
That's it.
Chào!
p/s: that's how i say bye in Vietnamese. ^^
And nest scribe is............................................Socola. ok? :D
Today we learned about rate law, reaction order, and calculating rate order. We did example 2 on page 28 in the blue booklet. For homework, we have to do page 32, 33, and part B on page 34.
That's it.
Chào!
p/s: that's how i say bye in Vietnamese. ^^
And nest scribe is............................................Socola. ok? :D
Sunday, April 11, 2010
DOUBLE DOWN!
Kay so this is a double blog post, cause I thought someone else posted but they didn't and then some things happened, it involved some elephant and a penguin... but I digress. Anyways, don't mind my memory lapse and this late blog.
On Thursday we were taught how to do average rate, you know
Rate = [(final concentration of A) - (initial concentration of A)] / [(final time) - (initial time)]
In other words:
Rate = [A]f - [A]i / Tf - Ti
Or in other words besides that:
Rate = Δ[A] / ΔT
We also learned about instantaneous rate: The rate at a specific time. The example is shown on page 12 and is answered in steps on page 13.
** by the way - the use of [A] can be replaces by any other variable [B], [C], [...]
We also went over:
Kinetics Assignment #1 Answers q. 1-3
On Friday (April 9th) We learned about Rate and Stoichiometry. The example on page 14 shows:
2NO2(g) -> 2NO(g) + O2(g)
We gave 2NO2(g) the value of 4g/min To find out the values of 2NO(g) and O2(g) we use ratios. 2NO2(g) and 2NO(g) have a ration of 2:2 or 1:1 so they have the same value, however O2(g) has a different concentration or ratio of 2:1 so it's 1/2 the amount of 2NO2(g) so it has 2g/min... get it?
We also created / answered some questions on Reaction Rate graphs. (Chapter 18 Worksheet)
(Sorry picture was too blurry... just google it or do your work :D !)
We also did all of the questions on page 15
Received Chapter 18 Worksheet or Reaction Rates Worksheet
Answered Questions 4 and 5 on Kinetics Assignment #1
Was assigned and corrected Questions 1-7 in Kinetics Assignment #2
** AND I THINK WE HAVE A CHEM TEST TOMORROW (April 12) ... I MAY BE WRONG AND IT MAY BE ON WEDNESDAY! ... SO YEAH! **
Yeapp, that's pretty much it... I think I mixed up some events that occurred on those days, but ... whatever they're bound to happen ha. Now a parting gift:
The KFC Double Down - Inspired the post.
Next scriibe is HYCharang :P
On Thursday we were taught how to do average rate, you know
Rate = [(final concentration of A) - (initial concentration of A)] / [(final time) - (initial time)]
In other words:
Rate = [A]f - [A]i / Tf - Ti
Or in other words besides that:
Rate = Δ[A] / ΔT
We also learned about instantaneous rate: The rate at a specific time. The example is shown on page 12 and is answered in steps on page 13.
** by the way - the use of [A] can be replaces by any other variable [B], [C], [...]
We also went over:
Kinetics Assignment #1 Answers q. 1-3
On Friday (April 9th) We learned about Rate and Stoichiometry. The example on page 14 shows:
2NO2(g) -> 2NO(g) + O2(g)
We gave 2NO2(g) the value of 4g/min To find out the values of 2NO(g) and O2(g) we use ratios. 2NO2(g) and 2NO(g) have a ration of 2:2 or 1:1 so they have the same value, however O2(g) has a different concentration or ratio of 2:1 so it's 1/2 the amount of 2NO2(g) so it has 2g/min... get it?
We also created / answered some questions on Reaction Rate graphs. (Chapter 18 Worksheet)
(Sorry picture was too blurry... just google it or do your work :D !)
We also did all of the questions on page 15
Received Chapter 18 Worksheet or Reaction Rates Worksheet
Answered Questions 4 and 5 on Kinetics Assignment #1
Was assigned and corrected Questions 1-7 in Kinetics Assignment #2
** AND I THINK WE HAVE A CHEM TEST TOMORROW (April 12) ... I MAY BE WRONG AND IT MAY BE ON WEDNESDAY! ... SO YEAH! **
Yeapp, that's pretty much it... I think I mixed up some events that occurred on those days, but ... whatever they're bound to happen ha. Now a parting gift:
The KFC Double Down - Inspired the post.
Next scriibe is HYCharang :P
Thursday, April 8, 2010
KINETICS
hi there!! its me jeck. I'm suppose to scribe yesterday but I totally forget it even Ms. K reminds about it. I'm sorry about that and my apologies to my grammars.
Anyway, yesterday Ms. K shows as how catalyst work on the solution. Catalyst define as something that initiates or causes an important event to happen. Originally a term used in chemistry for the volatile (active) chemical in a formula. (http://dictionary.reference.com/browse/catalyst). In simple explanation it speeds up the reaction of the two aqueous solutions. As I said earlier Ms. k shows us how it works in the solution. Well it really works but there was a little problem happen. The point is catalyst really works on the solution.
Yesterday we did our lab too, the part 3 and also we answer the questions in the lab sheet.
Sorry guys but I'm really bad at this thing (blogging). I work till 11:30 so I totally forgot about it.
Anyway, yesterday Ms. K shows as how catalyst work on the solution. Catalyst define as something that initiates or causes an important event to happen. Originally a term used in chemistry for the volatile (active) chemical in a formula. (http://dictionary.reference.com/browse/catalyst). In simple explanation it speeds up the reaction of the two aqueous solutions. As I said earlier Ms. k shows us how it works in the solution. Well it really works but there was a little problem happen. The point is catalyst really works on the solution.
Yesterday we did our lab too, the part 3 and also we answer the questions in the lab sheet.
Sorry guys but I'm really bad at this thing (blogging). I work till 11:30 so I totally forgot about it.
Tuesday, April 6, 2010
April 05 and April 06 2010
Hey there! I am scribing for two days:
One is the day after the Spring Break, Monday, April 05, 2010.
In class, we continued our studies on Chemical Kinetics. We answered the assignment assigned to us before Spring Break which was to do the questions on page 10 of our booklet in Chemical Kinetics. You have to read the previous pages to understand the answers. Here are they: (note: the answers are my own words, Ms. K was too lazy to write hers on the board...)(oh yeah, it said that you have to show diagrams.. but I don't know how to show mine here so figure that one yourself. :)
1.) The increase of concentration of the reactants the faster the reaction to occur therefore, increasing the reaction rate.
2.) a.) Increase in temperature causes the molecules to move faster, therefore more collision. More collisions/reactions --> increase in reaction rate. Decrease in temperature does the opposite --> slower reaction.
b.) The larger or more exposed the particle means more surface area. More surface area means greater chance of collisions --> increase in reaction rate. Less surface area, you know, slower reaction.
c.) More pressure means less travelling space. Less travelling space means faster collisions among the molecules --> increase in reaction rate. Less pressure means more travelling space and the collisions won't occur as fast.
3.) Catalysts provides an easier path for the reaction to proceed. It lowers the activation energy of a reaction, so, more particles are able to surpass the activation energy required. These means more collisions and an increase in the reaction rate.
4.) a. ) i. is faster because in a solution, reaction will occur more quickly to the ions because they are free to move.
b.) ii is faster because Ag is hungrier for elections than Cu. This brings us back to our previous unit, Atomic Structure. Ag has a higher Electronegativity value than Cu, so it can attract more electrons than Cu... I think.
c.) i is faster because all elements in the solution are ions.
d.) ii is faster because all of the elements are in the same state, gaseous form.
By the way, we only spent half of the class; we were called down to the gym for a meeting with the principal.
The second day is today, April 06, 2010.
We did a lab... and that's pretty much it. It was about how elements involved, concentration of the elements, temperature, a catalyst and particle size affect the reaction rate. We only did two parts of the lab sheet, so expect that we will do more of it tomorrow.
Yay! Jeck, it's your turn. :)
One is the day after the Spring Break, Monday, April 05, 2010.
In class, we continued our studies on Chemical Kinetics. We answered the assignment assigned to us before Spring Break which was to do the questions on page 10 of our booklet in Chemical Kinetics. You have to read the previous pages to understand the answers. Here are they: (note: the answers are my own words, Ms. K was too lazy to write hers on the board...)(oh yeah, it said that you have to show diagrams.. but I don't know how to show mine here so figure that one yourself. :)
1.) The increase of concentration of the reactants the faster the reaction to occur therefore, increasing the reaction rate.
2.) a.) Increase in temperature causes the molecules to move faster, therefore more collision. More collisions/reactions --> increase in reaction rate. Decrease in temperature does the opposite --> slower reaction.
b.) The larger or more exposed the particle means more surface area. More surface area means greater chance of collisions --> increase in reaction rate. Less surface area, you know, slower reaction.
c.) More pressure means less travelling space. Less travelling space means faster collisions among the molecules --> increase in reaction rate. Less pressure means more travelling space and the collisions won't occur as fast.
3.) Catalysts provides an easier path for the reaction to proceed. It lowers the activation energy of a reaction, so, more particles are able to surpass the activation energy required. These means more collisions and an increase in the reaction rate.
4.) a. ) i. is faster because in a solution, reaction will occur more quickly to the ions because they are free to move.
b.) ii is faster because Ag is hungrier for elections than Cu. This brings us back to our previous unit, Atomic Structure. Ag has a higher Electronegativity value than Cu, so it can attract more electrons than Cu... I think.
c.) i is faster because all elements in the solution are ions.
d.) ii is faster because all of the elements are in the same state, gaseous form.
By the way, we only spent half of the class; we were called down to the gym for a meeting with the principal.
The second day is today, April 06, 2010.
We did a lab... and that's pretty much it. It was about how elements involved, concentration of the elements, temperature, a catalyst and particle size affect the reaction rate. We only did two parts of the lab sheet, so expect that we will do more of it tomorrow.
Yay! Jeck, it's your turn. :)
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