hey guys ok so i'm going to be doing the blog post for the past few classes since i forgot to do it last week =\.

ok so to begin,

by examining the change in amount of substance at a particular time or over a period of time, the rate of reaction can be determined. The representation of such a reaction may be seen as the following once recorded onto a graph:














In order to calculate the rate we would use the formula:
RATE =

(final concentration of A) - (initial concentration A)
__________________________________

final time - initial time

- OR -

RATE = [A]final - [A]initial

_________________________

[t]final - [t]initial

INSTANTANEOUS RATE: of a reaction at a specific time is determined by calculating the slope of the line tangent to the point on the concentration vs time curve.

We also learned two types of reactions, exothermic and endothermic.

EXOTHERMIC: the product possess less energy than the reactants, during the reaction heat is lost from the system and (delta)H is a negative value.

ENDOTHERMIC: the product possess more potential evergy than the reactants, this energy is absorbed from it's surroundings, increasing the system's energy content, giving a positive (delta)H value.

ok so thats pretty much what we have been duscussing, on monday Mrs. Kozoriz, wasn't there but the sub gave two worksheets one we finished in class (reaction rate 52; CHANGE IN H2O0 WITH TIME) and one we had to work on for the rest of the class (reaction rate 17; A model for reaction rates).

THE NEXT SCRIBE WILL BE........... hm........ lucky : *****Niwatori-san******

Monday November 3/08

HEY everyone!!!
I am truely sorry about the very late post, my internet was down and i couldnt do anything last night. ANYWHO,
Yesterday in class, was just a work period. We had to finish the analysis from the lab. And if you haven't done the lab yesterday was the chance.
Ms.k gave us a word search to do if we were done.
either than that, i don't really know what to right because it was just a work period.

Sorry Ms.K, i know you dont like these kinds of blogs, but i dont know what to write. (or in this case type)

christine will be be the next blogger =)

Experiment: Part I

Hello there!!

Okay, so what we did today is the experiment:

Factors affecting the rate of a reaction.
Materials:
24-well test plate
HCl Solution
Water
Zinc Nitrate Solution
Iron Nitrate Solution
Acetic Acid
Copper Nitrate Solution
Toothpicks

And a few pieces of the following:
Magnesium
Aluminum
Zinc
Copper
Iron

Part I:
1.) Add 20 drops of 3.0 moL/L HCl Solution to each of five wells of the 24-well test plate.
2.) Place a small piece of Mg in the first well, a piece of Al in the second, a piece of Zn on the third, a piece of Fe in the fourth, and a piece of Cu in the fifth.
3.) Observe and Record your observations.
Questions:
1.) What gas is produced? How do you know?
2.) Write a balanced equation to represent the reaction.
3.) Do all the metals take the same time to react?
4.) Rank all the metals in order of reactivity.
4.) Add 13 drops of water and 7 drops of 3.0 mol/L HCl solution to one well. Use the toothpick to stir the solution.
5.) Add 13 drops of water and 7 drops of 3.0 mol/L Acetic Acid to a second well. Stir.
6.) Add 20 drops of 1.0 mol/L aqueous Zn(NO3)2 solution to a third well, 20 drops of 1.0 mL/L Fe(NO3)3 to a fourth well, and 20 drops of 1.0 mL/L Cu(NO3)2 to a fifth well.
7.) Place a small piece of Mg in each of the five solutions.
8.) Observe and Record your observations.
Questions:
1.) What happened in each test tube? I dentify the products in each case.
2.) Write a balanced equation to represent each reaction.
3.) How much time does the Mg take to react in each solution?

The next blogger is Angela!