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Name: Justin
Status: educator
Grade: 9-12
Location: IL
Country: N/A
Date: July 2006

Question:
I have been reviewing answers from open-ended laboratory reports I assigned my students this past year. I think I may have confused them on the speed of a reaction versus the time to the endpoint of reactants. At this point, I need help articulating what these concepts are.

I assign an experiment involving a pellet of baking soda and powdered baking soda with vinegar. The masses of baking soda are the same, but I am trying to get across the idea that the one with the greater surface area will react faster than the pellet (this is where I think I led them astray).

The answers indicate that the powdered baking soda reacted faster. One student said that the reaction was just a fast in both but the powdered baking soda generated carbon dioxide faster. I now think this student may be correct.

This has me thinking that "faster" is confusing between spent reactants and the amount of time to react.

And then I confused myself. Here are the questions I am struggling with: Are all chemical reactions, on the molecular level at the same rate of speed, or do they differ? If yes, that seems unusual in nature. If no, what determines the rate of reaction (not time to reaction completion of available reactants)?



Replies:
Hi Justin,

In the case of your baking soda experiment, with all other factors being equal, the speed of the reaction of the baking soda with vinegar would be the same for both forms. As you were trying to teach, the powdered baking soda has more sites for the reaction to take place simultaneously. Thus, overall all of the powdered baking soda will react before the peletized form.

Chemical reactions however do not happen at the same speed. Other factors such as temperature, pH, etc. can have a tremendous affect on reaction speed. For instance, the reduction of Cr+6 to Cr+3 can take hours at pH 8, if the pH is < 2, the reaction occurs in seconds.

The powdered baking soda generated carbon dioxide at the same rate as the peletized form per equal moles of baking soda reacting. More moles react and generate more CO2

Bob Hartwell


Justin,

Think of the rate of reaction (at the molecular level) as being dependent on two things: a spatial factor (rate of collisions in the correct orientation) and energy. You can see this mathematically in the Arrhenius equation (where the spatial factor is sometimes split between rate of collisions and orientation).

This means that at the molecular level, if you can increase the rate of collisions (and presumably the collisions that are in the correct orientation), then the over-all rate of the reaction will speed up. Thus, if you take the same amount of substance, but have one in powder form and another in a compact lump, then the rate of reaction of the powder will be faster (more surface to volume, more collisions). You can see this if you react an antacid tablet with vinegar (no stirring, do not wait for it to completely dissolve) as opposed to the same antacid tablet ground really fine. This is also why coal mines are dangerous (because of the fine dust in the air), but charcoal is safe enough to cook with.

There are many macroscopic factors/actions that affect rate of collisions: stirring, solubility, concentration, particle size, etc. - and this might have been the source of the confusion. But if all of these are controlled, then the rate of reaction (molecular level) should be reflected in the total time of reaction completion.

Also at the molecular level, the rate of reaction will speed up if energy is supplied. Thus, most reaction should go faster if they are heated.

With regard to your particular experiment, the reaction of sodium hydrogen carbonate (baking soda) with acid (vinegar) is a very fast reaction in the first place, so you really have to be careful that you are mindful of factors that affect rate to see a difference. But it should work for you. I suspect that the students who thought that the reaction was just as fast in both cases might have ignored the time it took for the pellet to dissolve, or may not have been using the same amount of liquid. The other possibility is that the vinegar was the limiting reagent and could have been controlling the over-all speed.

Hope this helped.

Greg (Roberto Gregorius)


I am not quite sure what a "speed of reaction" means to you. Your students may not know what it means to you either, which will make it difficult for any of us to communicate. So I will begin by defining what it means to ME, and go from there.

Like any rate, a reaction rate is a change in something with time. Specifically, the rate of a chemical reaction is the time derivative of the concentration of the product species (actually, of the concentration raised to the power of its stoichiometric coefficient). In other words, for a reaction, say,

A -> B,

the reaction rate is defined as

rate = d[B]/dt,

where [B] is the concentration of the product species B. If a reaction creates some different number of molecules of B, say, two, as in

D -> 2B,

the reaction rate is

rate = d([B]^2)/dt,

where [B]^2 means the square of [B].

Many reactions change their rates as they proceed. Often the rate depends on the concentration of the starting materials; as these are depleted, the reaction rate drops. Sometimes reactions are autocatalytic, which means that the product accelerates the reaction: the rates of such reactions skyrocket after a little product is formed. Other reactions generate heat, which raises the temperature and accelerates the reaction. Many different things can happen!

Now, it is hard to measure a reaction rate directly. Usually what you can measure is the amount or concentration of one of the starting materials or products, and you need to estimate what the rate of its change is. If you can measure the change over some time interval, you can calculate the average reaction rate over that interval, as

average rate = (change in [B])/(elapsed time).

With your powdered baking soda, you and your students saw that powdered baking soda generated gas faster than the same mass of baking soda in tablet form. What is the reaction whose rate you are trying to assess? If the reaction is the generation of gas, then the system giving the faster gas generation is the system with the faster rate.

I do not think this actually answered your question because I do not believe I understand what it is you want to know. I hope this can give you a beginning, so that you can ask again in the hope that we can communicate more efficiently once we understand each other better.

Richard Barrans



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