Week 7 Question 2

With Exam 2 next Tuesday, identify one topic that is causing you issues from Chapter 13 or Chapter 14. The next person should address the issue and then list their own issue.

For example: In a given mechanism, how would I know which step is the slow step if they are not identified but the experimental rate law is?

Week 7 Question 1

We are going to ask questions for the following reaction according to Le Chatlier's Principle. I will start with a question, the next person should answer it and ask their own question.

                                        CaCO₃(s) ⇌  CaO(s)  +  CO₂(g)                 ∆H = 131.4 kJ

Explain what happens to the value of the equilibrium constant when CaO is added to the reaction at equilibrium.

Week 6

We are going to answer a question and ask a question in each posting. First you answer the previous post's question and then you ask your own question. Let's try to keep it mostly conceptual (some math allowed) so that we can get at what these concepts mean.

A dynamic equilibrium arises when the rate of a forward reaction becomes equal to the rate of the reverse reaction. This is a process that occurs very often in chemical reactions. The ratio of the rate constant for the forward reaction, kf to the rate constant for the reverse reaction, kr is called an equilibrium constant, K. Thus K = kf /kr. 

If the rate constant for the forward reaction equals 1.2x10³ and the rate constant for the reverse reaction equals 4.1x10², what would be the value for the equilibrium constant? What do you think this means in terms of whether there are more reactants or more products at equilibrium?

Week 5

I am going to choose a term or a process from the Kinetics chapter (Chap 13) and explain it. The next person to post will give either an example or an illustration (an analogy about the concept). The next person will choose another term or process and we will keep alternating back and forth between an explanation and an example/illustration.

Starting:

Temperature impacts the rate of a reaction through increasing the speed of the molecules, which in turn increase the number of collisions. An increase in the number of collisions increases the probability that a reaction will occur since according to the Collision Theory, molecules have to collide (or nearly) in order for a reaction to occur between molecules.

Now the next person, give an example or an analogy!
After that the third person will explain another term and we will alternate back and forth.

Week 4 Question 2

Follow the link and read the article. Comment on at least one topic relating to chemistry.

http://alternativefuels.about.com/od/environmentalimpact/a/winterfuelecon.htm

Week 4 Question 1

4 NH₃(g)  + 5 O₂(g)   --->   4 NO(g)  +  6 H₂O(l)

I will write a question based upon rates of the above reaction. The first person will answer this question and then write a second question that the next person will answer and then write a question continuing on …..

So to start: What is the expression for the rate of disappearance of NH₃?