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.
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.
An analogy for temperature impacting the rate of a reaction can be people going to the beach. As the temperature increases more people are likely to go to the beach which increases the chance of people bumping into each other or interacting with one another (the reaction). And as the temperature decreases less people will go to the beach resulting in the less likelihood of people bumping into each other or interacting with one another (the reaction).
ReplyDeleteA catalyst is a substance that increases the rate of a chemical reaction without itself being permantently changed. From the equation, k = Ae^−(Ea/RT), a homogeneous catalyst typically decreases the value of Ea, or activation energy, by providing an alternate pathway for the reaction to take place. A heterogeneous catalyst typically increases the value of A by acting a a reaction site, bringing the reactants together for the reaction to occur. In either case the rate constant would be increased.
ReplyDeleteThanks for your responses!
ReplyDeleteIf you look at a reaction like a road that cars go down their a few analogies for a catalyst. A homogeneous catalyst might be something like a more aerodynamic car. While the design will not change throughout the drive (reaction) it will decrease the amount of gas needed to get to it's destination (decease activation energy). a heterogeneous mixture might be something like opening up a new highway which gives you more ways to get to your destination or ways to meet up with fellow cars.
ReplyDelete