Department of Energy Argonne National Laboratory Office of Science NEWTON's Homepage NEWTON's Homepage
NEWTON, Ask A Scientist!
NEWTON Home Page NEWTON Teachers Visit Our Archives Ask A Question How To Ask A Question Question of the Week Our Expert Scientists Volunteer at NEWTON! Frequently Asked Questions Referencing NEWTON About NEWTON About Ask A Scientist Education At Argonne Endo, Exothermic Reactions and Energy
Name: Emily M.
Status: student
Age: 14
Location: N/A
Country: N/A
Date: Sunday, February 23, 2003


Question:
What is the difference between an endo and exothermic reaction. What are some examples? Like where does the energy for each come from? I am told the energy is in the chemical bonds, but I am also told that a bond is at low potential. It cannot be at high and low energy at the same time. Please help!


Replies:
An endothermic reaction absorbs heat from its surroundings; an exothermic reaction releases heat into its surroundings. If a reaction running in one direction is endothermic, the reverse direction is exothermic. Often, the "spontaneous" direction of a reaction, that is, the direction it will go if it can go any direction at all, is the exothermic direction.

An example is dissolving sodium hydroxide in water. Sodium hydroxide spontaneously dissolves in water and releases heat in the process. A solution of sodium hydroxide in water does not readily separate into pure water and solid sodium hydroxide. Another example of an exothermic reaction is the combustion of hydrogen gas with oxygen to produce water and heat.

An example of a spontaneous endothermic reaction is dissolving ammonium nitrate in water. Just as with sodium hydroxide, ammonium nitrate is very soluble in water. In contrast to sodium hydroxide, when ammonium nitrate dissolves the solution gets colder, that is, it absorbs heat. Another endothermic reaction is the reaction of baking soda and vinegar to make carbon dioxide and sodium acetate.

"Where does the energy come from" is a simple question, but the answer is somewhat complex. I suspect that the answer will also be a lot longer than you would like it to be. It turns out that it is not actually energy that drives a chemical reaction, but instead a quantity called "entropy."

I find it hard to understand a rigorous definition of entropy, but I can give you an example. Let us say that a swimming pool is filled with plain water. I place a balloon filled with blue dye into the pool and pop the balloon. What happens to the blue dye? It slowly mixes with the rest of the water in the pool. Why? The dye molecules are constantly moving around, bouncing off each other and off the water molecules. They can bounce back into where the balloon used to be, or they can move into places where they were not before. If they have no reason to go in one direction instead of another, where will they go? They can move to any place in the pool. There is no preference for any one place over another. So, they will eventually spread out to color the entire pool, not because they are acting together, but because they each individually move in any direction.

Will the dye molecules ever spontaneously move back to where they started, that is, where the balloon used to be? Yes, actually, each individual dye molecule will, if given enough time, at some time occupy every location in the pool. Will all the dye molecules ever spontaneously move back to where the balloon used to be, all at the same time? Doing this would amount to running the reaction backward: all the dye molecules unmix from the pool water and go back into one spot. You probably know that this will not happen, but why will it not? Here is why. The volume of the balloon is only a very small fraction of the total volume of the pool. Let's call this fraction b. This fraction b is less than 1 and greater than zero. At any time, the probability that any given dye molecule is where the balloon used to be is b. For the reaction to run backwards, all of the dye molecules would need to be in that region. IF there are N dye molecules, the probability that this will happen is b^N, that is, b times itself N times. In chemical systems of any significant size, N is a very large number, larger than billions and larger than trillions. So b^N is an infinitesimally small probability, so close to zero that as far as we can observe it IS zero. Thus we can say that dye mixed throughout the water in a pool will NOT spontaneously unmix and concentrate in a small volume.

The reason I went through that long example was to explain the principle behind entropy. "Entropy" is a way to measure the tendency of systems to arrange themselves so that making many small deviations will not change the arrangement much. In the swimming pool example, moving the dye molecules around when they are already dispersed throughout the water will not make things look very different. When they are close together in a small region, though, moving them around will have a bigger relative effect.

There are two basic ways that entropy can increase in a reaction:

* The reaction can give off heat. Heat means that molecules are moving faster, enabling them to move into many different arrangements rapidly.

* The reaction can transfer molecules from a restricted to a free state. This is what happens when solids dissolve in liquids, or gases are produced.

In the swimming pool example, the dye molecules go from a restricted state (inside to balloon) to a freer state (dispersed throughout the pool). Heat transfer is not important here.

When sodium hydroxide dissolves in water, heat is given off AND solid sodium hydroxide becomes freely mobile in the water. This is a very favorable reaction.

When ammonium nitrate dissolves in water, the solid ammonium nitrate becomes more mobile, but the solution absorbs heat. These two processes oppose each other, and the winner is the increased mobility of the ammonium nitrate.

The same battle of tendencies occurs in the baking soda + vinegar reaction. Carbon dioxide gas is produced, which is much more mobile than the baking soda or vinegar. This increased mobility overcomes the unfavorable influence of absorbing heat.

I am almost done answering your questions. You last question concerned whether the energy of reactions comes from breaking chemical bonds. That question was answered in great detail by a number of scientists (including me) earlier. The link to the question and its replies is at

http://www.newton.dep.anl.gov/askasci/gen99/gen99928.htm

Richard E. Barrans Jr., Ph.D.
PG Research Foundation, Darien, Illinois



Click here to return to the Chemistry Archives

NEWTON is an electronic community for Science, Math, and Computer Science K-12 Educators, sponsored and operated by Argonne National Laboratory's Educational Programs, Andrew Skipor, Ph.D., Head of Educational Programs.

For assistance with NEWTON contact a System Operator (help@newton.dep.anl.gov), or at Argonne's Educational Programs

NEWTON AND ASK A SCIENTIST
Educational Programs
Building 360
9700 S. Cass Ave.
Argonne, Illinois
60439-4845, USA
Update: June 2012
Weclome To Newton

Argonne National Laboratory