collision theory gizmoDONE.2022-2023

collision theory gizmoDONE.2022 collision theory gizmoDONE.2022

Name: ______________________________________ Date: ________________________

Student Exploration: Collision Theory

NCVPS Chemistry Fall 2014

Vocabulary: activated complex, catalyst, chemical reaction, concentration, enzyme, half-life,

molecule, product, reactant, surface area

Prior Knowledge Questions (Do these BEFORE using the Gizmo.)

1. Suppose you added a spoonful of sugar to hot water and another to ice-cold water. Which

type of water will cause the sugar to dissolve more quickly? Hot water.

2. Suppose you held a lighted match to a solid hunk of wood and another match to a pile of

wood shavings. Which form of wood will catch fire more easily? Wood shavings.

Gizmo Warm-up

A chemical reaction causes the chemical compositions

of substances to change. Reactants are substances that

enter into a reaction, and products are substances

produced by the reaction. The Collision Theory Gizmo™

allows you to experiment with several factors that affect

the rate at which reactants are transformed into products

in a chemical reaction.

You will need blue, green, and orange markers or colored

pencils for the first part of this activity.

1. Look at the key at the bottom of the SIMULATION pane. In the space below, draw the two

reactants and two products of this chemical reaction.

Reactants: A Products: A

B

B

2. Click Play ( ). What do you see? The first three were reactants A and B but reactants

A took part of reactants B and then turned into products A and B.

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Activity A:

Temperature

Get the Gizmo ready:

 Click Reset ( ).

 Check that the Reactant concentration is set to

1.0 mol/L, the Catalyst concentration is set to

0.00 mol/L, and the Surface area is Minimum.

Question: How does temperature affect the rate of a chemical reaction?

1. Observe: Select the ANIMATION tab. View the animation with No catalyst selected.

What do you see? the higher the temperature, the faster the chemical reaction.

When two reactant molecules meet, they form a temporary structure called an activated

complex. The activated complex breaks up into the product molecules.

2. Observe: Return to the CONTROLS pane. Set the Temperature to 0 °C and the Simulation

speed to its maximum setting. Click Play.

A. Describe the motions of the molecules. They slow down.

B. Now set the Temperature to 200 °C. How does increasing the temperature affect the

motions of the molecules? They speed up.

C. What do you notice about the chemical reaction at the higher temperature? The

chemical reactions become faster.

3. Interpret: Select the GRAPH tab. Click the zoom out button ( ) until you can see the whole

graph. What does this graph show? The reactants go down and the products go up.

4. Predict: How do you think temperature will affect the rate of a chemical reaction? The

reaction will happen in a shorter amount of time if the temperature is up.

(Activity A continued on next page)

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Activity A (continued from previous page)

5. Gather data: Click Reset. A useful way to compare reaction rates is to record the time

required for half of the reactants to react, called the half-life of the reaction. With the

Temperature set to 200 °C, click Play. Click Pause ( ) when the number of reactant

molecules is 10. Record the half-life time in the first space of the table below.

Trial 200 °C 150 °C 100 °C 50 °C

1 5:42 7:04 12:02 45:02

2 4:42 7:02 20:42 48:02

Mean half-life 5:32 7:03 16:22 46:52

Repeat the experiment at different temperatures to complete the table. (Note: To get exact

times, you can refer to the TABLE tab.)

6. Calculate: Calculate the mean half-life for each temperature. Fill in these values above.

(Hint: To get an exact mean, first convert each time to seconds by multiplying the minutes

value by 60 and adding this to the seconds. To find the mean in seconds, add up the two

times and divide by two. Convert the answer back to minutes and seconds.)

7. Analyze: What do your results indicate? As the temperature goes down, the time goes up.

8. Draw conclusions: For two molecules to react, they must collide at just the right angle and

with enough energy to break the original bonds and form new ones. Based on these facts,

why does the reaction tend to go more quickly at higher temperatures?

At a higher temperature, the molecules move faster so they can more of a chance of hitting

each other at just the right angle.

9. Apply: Paper must be heated to 234 °C to begin reacting with oxygen. This can be done by

putting the paper over a flame. Why do you think the paper must be heated to start burning?

Even though the paper is put over a flame, it still needs time to react or for the molecules to

hit each other just right.

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Activity B:

Surface area and

concentration

Get the Gizmo ready:

 Click Reset.

 Check that the Catalyst concentration is set to

0.00 mol/L and the Surface area is Minimum.

 Set the Temperature to 200 °C.

Introduction: Reaction rates are also influenced by surface area and concentration. The

surface area of a solid is a measure of how much of the solid is exposed to other substances.

The concentration of a substance is a measure of how many molecules of that substance are

present in a given volume.

Question: How do surface area and concentration affect reaction rates?

1. Observe: Change the Surface area from Minimum to Maximum. How does this change

the amount of Reactant B molecules that are exposed to Reactant A?

They are moving around and not staying on one side.

2. Predict: How do you think increasing the surface area will affect the rate of the reaction?

It will make the reaction go faster.

3. Gather data: Set the Reactant concentration to 2.0 mol/L. Use the Gizmo to measure

the half-life of the reaction for each surface area setting. (There will now be 20 reactant

molecules left at the half-life.) Then, calculate the mean half-life for each setting.

Trial Minimum surface area Maximum surface area

1 3:32 1:22

2 4:22 0:22

Mean half-life 4:17 1:12

4. Analyze: What do your results indicate? Most surface area speeds up the process of the

chemical reaction.

5. Explain: Why does the reaction proceed more quickly when the surface area is

increased?

The reactants B are spread out so they don’t have to wait for a reactant A to come get them

and they are moving.

(Activity B continued on next page)

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Activity B (continued from previous page)

6. Observe: Click Reset. Move the Reactant concentration slider back and forth. What do

you notice?

With more reactant, it’s easier for them to find each other.

7. Predict: How will increasing the reactant concentration affect the rate of the reaction?

Why?

A higher concentration will make the reaction longer because there is more to react.

8. Gather data: Make sure the Temperature is 200 °C and the Surface area is Maximum.

Use the Gizmo to measure the half-life for each given reactant concentration. (Note that the

number of reactant molecules changes with each concentration.) Calculate the means.

Trial 0.4 mol/L 0.8 mol/L 1.2 mol/L 1.6 mol/L 2.0 mol/L

1 10:00 2:54 1:58 1:08 1:10

2 8:24 2:04 2:26 1:18 0:46

Mean half-life 9:12 2:58 2:12 1:32 0:58

9. Compare: If possible, find the mean times for each concentration for your entire class.

What is the mean class time for a concentration of 0.4 mol/L? How about for 2.0 mol/L?

Mean for 0.4 mol/L: ? Mean for 2.0 mol/L: ?

10. Analyze: What do these results indicate? More concentration will equal a faster result.

11. Apply: Hydrochloric acid reacts with the mineral calcite to produce carbon dioxide gas,

water, and calcium chloride. Based on what you have learned in activity A and activity B,

what are three things you could do to make the reaction occur more quickly?

Increases the temperature, surface area, and the reactant concentration.

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Activity C:

Catalysts

Get the Gizmo ready:

 Click Reset ( ).

Introduction: A catalyst is a substance that helps a chemical reaction to proceed. The catalyst

molecules are not changed by the reaction and can be reused over and over again.

Question: How do catalysts affect the rate of a chemical reaction?

1. Observe: Select the ANIMATION tab. Select With catalyst and observe.

A. What do you see? reactants transfer atoms inside the catalyst.

B. Why do you think the shape of a catalyst is important? To help them transfer an

atom.

Many catalysts have a special shape that allows them to bind to specific reactant molecules.

2. Predict: How do you think catalysts will affect the rate of a chemical reaction? Increase

the rate.

3. Gather data: On the CONTROLS pane, set the Reactant concentration to 2.0 mol/L, the

Surface area to Maximum, and the Temperature to 50 °C. Measure the half-life for each

given catalyst concentration. Calculate the means.

Trial

Catalyst concentration

0.00 mol/L 0.05 mol/L 0.10 mol/L 0.15 mol/L

1 35:02 4:46 2:06 1:12

2 28:02 3:10 2:0 1:11

Mean half-life 31:32 3:58 2:18 1:11

4. Analyze: What do your results indicate? If there are more catalyst, then you will have a

faster result.

(Activity C continued on next page)

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Activity C (continued from previous page)

5. Explore: Set the Catalyst concentration to 0.00 mol/L and the Temperature to 0 °C.

Click Play, wait for 10 minutes of simulated time, and click Pause.

A. What happens? 6 products were formed.

B. Click Reset, set the Catalyst concentration to 0.25 mol/L, and click Play. After 10

simulated minutes, click Pause. What happens now? 36 products were formed.

C. Why do you think the catalysts allowed the chemical reaction to take place at 0 °C?

They add energy.

6. Draw conclusions: What is the usefulness of catalysts? They speed up reactions and

assist to guide.

7. Apply: Most of the chemical reactions inside your body rely on protein catalysts called

enzymes to take place. For example, the enzyme pepsin helps to break down protein

molecules in your stomach. What might happen if your stomach stopped producing pepsin?

Protein molecules would not be broken down.

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