Pull Back the Knob. What Happened Reaction & Rates Lab Report


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Guided Inquiry # 5

Chemical Kinetics (Rate of Reaction)

Four major things affect the rate of a reaction:


More molecules more collisions

Collisions are necessary for reactions

Physical State:

Ability to mix reactants

Solids can be grinded to increase surface area Liquids can be stirred

Tem erature:

Increases the kinetic energy of molecules

Need sufficient energy to react (Activation Energy)


Typically lower the activation energy of reactions

For the majority of this guided inquiry we are going to use a simulation program written by Linda Koch, Ron LeMaster, Trish Loeblein, and Kathy Perkins. The program can be found by following this link:



Opening the program from the course’s moodle site under Guided Inquiries

Reactions & (1.07)

Single Collision

Pull back the knob. What happened? (Discuss with your partner(s) or to yourself)

Click the “Reload Launcher” button and expand the two windows on the right side of the program by clicking the “+” button for the Separation View and the Energy View. Now release the knob from various distances.

Indicate on the potential energy diagram when the reaction proceeds forward.

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Reaction Coordinate

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Now click the Angled Shot option in the top right comer.

Try launching from a different angle or two.

Did the reaction proceed as before?

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Why do you think this was the outcome despite having enough energy for the reaction to proceed?

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Set the Choose a reaction option to the last preset chemical reaction that isn’t Design your own.

Now Change the Launcher Options back to Straight Shot and release the knob.

What happens to the translational speed of the molecules as the reaction goes forwards and backwards? (Hint: the effect will be easiest to observe at a low energy) Please explain why this occurs.

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Click on the “Rate Experiments” tab found at the top middle of the program window.

Set Options (bottom right corner) to Strip.

Increase the Initial Temperature (right side of window) until the Average Energy (green bar) is equal to the potential energy of the product

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Set each reactant to l .

How much time does it take to react?

(Stop if it has been 2 minutes or roughly 3000 seconds on the programs graph)

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If no reaction occurred, stop the reaction after 2 minutes and increase reactant by l . Repeat until the reaction occurs.

How many reactants had to be used?

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Explain how this reaction took place below the activation energy?

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Now start out with 5 of each reactant.

Record how long it takes for I reaction to take place (The program counter will suffice).

Repeat the experiment for a total of 5 times.

Then throw out the fastest and slowest time and average the remaining 3 experiments.

5 Reactants Each

Run l : Average:

Run 2:

Run 3:

Run 4:

Run 5:

word image 3193 Repeat this process for 10 reactants each and 15 reactants each.

Run l :

Run 2:

Run 3:

Run 4:

Run 5:

10 Reactants Each


Run l :

Run 2:

Run 3:

Run 4:

Run 5:

15 Reactants Each


How did the rate of the reaction change?


To find the rate law of a reaction, a minimum of two experiments will have to be perforrned where only one reactant’s initial concentration is changed. This will allow you to determine the order of the reaction for that particular reactant.

Rate = kword image 3194

Finding Order of the Reaction for a Reactant and Rate Constant



N02 NO + -02


Rate M/S

Run I



Run 2



Run 3

I .60

I .38

Using Run I & 3:

1.60 M

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1 38 M/

= 3.54

0.85 M word image 3196

0.39 M/S word image 3197

(1.å8)X 3.54

xln 1.88 = In 3.54

In 3.54

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In 1.88

x = 2. 0025 Round to nearest whole number or multiply by two then round word image 3199

Find Rate Constant

Using Run 3:

(Rate)o 1.38 M/S 1.38 M/S k = 0.539 M word image 3200

[N02]2 (1.60 M) 2.56 M 2

Find Rate Law

(Rate)o = 0.539 M -l s word image 3201


Find the Rate Law given the following information.


NO +- Br2 NOBr


Rate (M/

Run I


I .00

1.30 x lo-

Run 2


I .00

2.93 x lo-

Run 3



8.78 x IO-

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