chemical reactions idr 10 16 14 - lablearner...10.question: how do you know that a chemical reaction...

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Chemical Reactions Investigation Two

Data Record Name: Date: 1. During this Investigation, you will analyze how changing the amounts of

the reactants in a chemical reaction affects the amount of the products that are produced. By performing the experiments in the Investigation, you will answer the following questions:

Focus Questions:

In a chemical reaction, do the amounts of the reactants affect the amounts of products produced? How does the Law of Conservation of Matter relate to chemical reactions?

Tool: Prediction You are going to study how changing the amount of the reactants affects the amount of the products of a chemical reaction. Use the Prediction tool to think of possible answers to the following questions: • Are the reactants always completely used up in a chemical reaction?

Student answers may vary. • Does the matter making up the reactants disappear?

Student answers may vary. • What happens if there is more of one reactant than the other reactant?

Student answers may vary. • How do you know when a chemical reaction has stopped?

Student answers may vary.


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2. Materials per group: • 1 triple beam balance

• 1 500 ml Erlenmeyer flask

• 1 lab scoop

• 1 weigh dish

• 6 large balloons

• 1 15 ml centrifuge tube

• 1 100 ml graduated cylinder

• 3.5 g of Magnesium (Mg)

powder

• 1 400 ml beaker

• 350 ml of hydrochloric acid

(HCl) in a beaker

• 1 metric ruler

• 1 calculator

• 1 stop watch

• 1 pair gloves per student

• 1 pair goggles per student


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3. Procedural Toolbox

During each Trial in this Investigation, you will use the following tools from the Procedural Toolbox.

Triple Beam Balance Equilibration Triple Beam Balance Use and Operation Measuring Mass Using a Weigh Dish or Beaker Graphing of Independent and Dependent Variables

Background In a chemical reaction, the chemical bonds that hold the atoms of the reactants together are broken and reformed in a different arrangement to form the products. Breaking and reforming these bonds occurs when the reactants react with each other. The different arrangement of atoms can be seen by the different formulas that represent the reactants and products. When all of the reactants are consumed in a chemical reaction, they no longer exist in their original form. All the atoms originally found in the reactants can now be found in the products. The observation that all the matter of the reactants is converted into the matter of the products is referred to as the Law of Conservation of Matter. Sometimes two reactants are not present in equivalent or equal amounts. More of one reactant is present compared to the other. The reactant present in the lesser amount is completely consumed or used up in such a chemical reaction. Since none of this reactant remains, the chemical reaction must stop. When the reaction stops, only a portion of the other reactant has been consumed, meaning that some is still unreacted. In this Investigation, the following chemical reaction will take place. Mg + 2 HCl → MgCl2 + H2

Magnesium Metal

Hydrochloric Acid

Magnesium Chloride

Hydrogen gas


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Experiment 1. Six Trials will be performed in this Investigation. The first 5 Trials will

use the same mass of magnesium metal (Mg) but a different volume of hydrochloric acid (HCl). The last Trial will use a different mass of magnesium (Mg). In all Trials, the amount of one of the products, hydrogen gas, will be determined. Use Table A as a guide for the mass of magnesium (Mg) and the volume of hydrochloric needed for each Trial.

Table A

Trial Mass of Mg (g)

Volume of HCl (ml)

1 0.5 2 2 0.5 15 3 0.5 50 4 0.5 75 5 0.5 100 6 1 100

Trial 1 1. In this Trial you will investigate the reaction of 2 ml of hydrochloric acid

(HCl) with 0.5 g of magnesium.

a. Use the centrifuge tube to measure 2 ml of HCl and add it to the Erlenmeyer flask.

b. Use the triple beam balance, lab scoop, and weigh dish to measure 0.5g of magnesium. If you need help, read the Procedures, Triple Beam Balance Equilibration, Triple Beam Balance Use and Operation, and Measuring Mass Using a Weigh Dish or Beaker.

Mass of weigh dish 5.0 g

Mass of weigh dish and magnesium 5.5 g

c. Blow up each balloon to stretch and then deflate it. Use the lab scoop to add the 0.5g of magnesium to a balloon.


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d. Stretch the open end of the balloon over the mouth of the Erlenmeyer flask until it securely covers the mouth of the flask. During this step, do not allow any magnesium metal to fall into the flask.

e. Use the triple beam balance to determine the total mass of the flask, hydrochloric acid (HCl), balloon, and magnesium.

2. Record: Write the mass for “Before Reaction” in Table B.

Table B

Mass of Flask, HCl, Mg and balloon (grams)

Before Reaction 204 After Reaction 204

3. Making sure that the balloon does not come off the mouth of the flask,

hold the balloon and shake the magnesium out of the balloon until all of it has fallen to the bottom of the flask into the hydrochloric acid (HCl).

4. Gently swirl the flask, so the magnesium stays in contact with the

hydrochloric acid. After approximately 5 minutes, the production of the product, hydrogen gas (H2), will have stopped. Do not remove the balloon.

5. Using the triple beam balance, determine the total mass of the flask,

hydrochloric acid (HCl), balloon, and any remaining magnesium metal. 6. Record: Write the mass for “After Reaction” in Table B. 7. Question: What was the mass of the flask, hydrochloric acid (HCl),

balloon, and magnesium metal (Mg) before the reaction?

Student answers may vary.


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8. Question: What was the mass of the flask, hydrochloric acid (HCl), balloon, and magnesium (Mg) after the reaction? Was it the same as the mass of the flask, hydrochloric acid, and magnesium before the reaction?

Student answers may vary. Yes, the mass should be the same as the

mass before the reaction took place.

9. Question: Do the data support the Law of Conservation of Matter? Why?

Student answers will vary. Yes, the Law of Conservation of Matter was

supported because the total mass of the flask, hydrochloric acid (HCl),

and balloon was the same before and after the reaction.

10. To determine how much hydrogen gas (H2) was produced, use the metric

ruler to measure the diameter of the balloon in centimeters. The diameter is the distance across the width of the balloon.

11. Record: Enter the diameter of the balloon in Table C in the row for Trial

1. Table C is located after Trial 6 in the Student Data Record. 12. Question: What was the product of the reaction that caused the balloon

to expand? (Hint: look at the chemical equation in the Background)

The product of the reaction was hydrogen gas (H2) 13. Question: How do you know that a chemical reaction occurred?

One of the products of the reaction is hydrogen gas (H2). The balloon

attached to the flask expanded as it filled with the hydrogen gas (H2)

produced by the chemical reaction.


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14. Question: Did any magnesium (Mg) remain after the reaction ended?

Yes, some magnesium remained. 15. Discard the contents of the flask in the 400 ml beaker, and rinse the flask

with water. Trial 2 1. In this Trial you will investigate the reaction of 15ml of hydrochloric acid

(HCl) with 0.5g of magnesium.

2. Question: Do you think the balloon will expand to a smaller or larger

diameter in Trial 2 compared to Trial 1. Explain the reason for your prediction. The balloon will expand to a greater diameter than in Trial 1. More

hydrogen gas (H2) will be produced because more hydrochloric acid

(HCl) reactant is used.

3. Using the 100 ml graduated cylinder, measure 15ml of hydrochloric acid

(HCl) and add it to the Erlenmeyer flask. 4. Use the triple beam balance, lab scoop, and weigh dish to measure 0.5g

of magnesium. Add the 0.5 g of magnesium to a new balloon. 5. Stretch the open end of the balloon over the mouth of the Erlenmeyer

flask until it securely covers the mouth of the flask. During this step, do not allow any magnesium to fall into the flask.

6. Making sure that the balloon does not come off the mouth of the flask,

hold the balloon and shake the magnesium out of the balloon until all of it has fallen to the bottom of the flask into the hydrochloric acid.

Tool: Prediction Use the Prediction tool to answer the following question.


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7. Gently swirl the flask so the magnesium stays in contact with the hydrochloric acid. After approximately 5 minutes, the production of the hydrogen gas will have stopped. Do not remove the balloon.

8. To find out how much hydrogen was produced, use the metric ruler to

measure the diameter of the balloon in centimeters. 9. Record: Enter the diameter of the balloon in Table C in the row for Trial

2. Table C is located after Trial 6 in the Student Data Record. 10. Question: How do you know that a chemical reaction occurred?

One of the products of the reaction is hydrogen gas (H2). The balloon

attached to the flask expanded as it filled with the hydrogen gas


11. Question: Did any magnesium remain after the reaction ended?

Yes, some magnesium (Mg) remained. 12. Question: Why did the balloon expand to a smaller or larger diameter

compared to Trial 1?

More of the reactant, hydrochloric acid, was used in Trial 2 so more of

the product, hydrogen gas (H2), was produced.


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Trial 3 1. In this Trial you will investigate the reaction of 50ml of hydrochloric acid

(HCl) with 0.5g of magnesium.


diameter compared to Reaction 2? Explain the reason for the prediction.

The balloon will expand to a greater diameter than in Trial 2. More

hydrogen gas (H2) will be produced because more hydrochloric acid

(HCl) reactant is used.

3. Repeat the procedure used for Trial 2 using 50 ml of hydrochloric acid

and 0.5g of magnesium. 4. Record: Enter the diameter of the balloon for Trail 3 in Table C. 5. Question: How do you know that a chemical reaction occurred?

One of the products of the reaction is hydrogen gas. The balloon

attached to the flask expanded as it filled with the hydrogen gas


6. Question: Did any magnesium remain after the reaction ended?

Student answers may vary. No magnesium remained. 7. Question: Did the balloon expand to a smaller or larger diameter

compared to Trial 2?

The balloon expanded to a greater diameter than in Trial 2.



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Trial 4 1. In this Trial you will investigate the reaction of 75ml of hydrochloric acid

with 0.5g of magnesium.


diameter compared to Trial 3. Explain the reason for your prediction.

Student answers will vary. The balloon will expand to the same

diameter compared to Trial 3 because all of the magnesium will be used

up.


and 0.5g of magnesium. 4. Record: Enter the diameter of the balloon for Trial 4 in Table C. 5. Question: Did any magnesium remain after the reaction ended?

Student answers may vary. No magnesium remained.

6. Question: Did the balloon expand to the same diameter as in Trial 3?

The balloon expanded to the same diameter as in Trial 3.



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Trial 5 1. In this Trial you will investigate the reaction of 100ml of hydrochloric

acid with 0.5g of magnesium.

2. Question: Predict whether the balloon will expand to a smaller or larger

diameter compared to Trial 4. Explain the reason for your prediction.

Student answers will vary. The balloon will expand to the same

diameter compared to Trial 3 because all of the magnesium will be used

up.


and 0.5g of magnesium. 4. Record: Enter the diameter of the balloon for Trial 5 in Table C. 5. Question: Did any magnesium remain after the reaction ended?

Student answers may vary. No magnesium remained. 6. Question: Did the balloon expand to the same diameter as in Trial 3?

The balloon expanded to the same diameter as in Trial 3.



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Trial 6 1. In this Trial you will investigate the reaction of 100ml of hydrochloric

acid with 1 g of magnesium.


diameter compared to Trial 5. Explain the reason for the prediction.

Student answers will vary. The balloon will expand to a larger diameter

because more magnesium will be used in this trial

3. Repeat the procedure used for Trial 2 using 100 ml of hydrochloric acid and 1 g of magnesium.

4. Record: Enter the diameter of the balloon for Trial 6 in Table C. 5. Question: Did the balloon expand to a smaller or larger diameter than in

Trial 5?

The balloon expanded to a larger diameter than in Trial 5.

Table C

Trial Mass of

Mg (g)

Volume of HCl (ml)

Diameter of Balloon

(cm)

Volume of Balloon

(ml) 1 0.5 2 4 33.3 2 0.5 15 5.75 98.9 3 0.5 50 8.5 319.3 4 0.5 75 8.5 319.3 5 0.5 100 8.5 319.3 6 1 100 10 520



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Analysis 1. Before the data can be analyzed, the amount of hydrogen gas that was

produced as a product must be determined for each reaction. This can be done by calculating the volume of the inflated balloon for each reaction.

a. Since the balloon is a sphere, use the formula for the volume of a

sphere.

In the following equations: π = 3.14 r = the radius of a sphere in centimeters d = the diameter of a sphere in centimeters d3 = (d • d • d)

The volume of a sphere = 4 • π • r3

3

This can be simplified to: Volume of a sphere = 0.52 • d3 = 0.52 • (d • d • d)

b. In the space below, use the measured diameter of the balloon in each

reaction to calculate the volume of H2 gas produced. c. Enter the calculated volumes in the last column of Table C.


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2. Graph: Use the axes below to draw a graph that compares the concentration of volume of hydrogen gas (H2) that is produced to the volume of hydrochloric acid (HCl) used. Use the data from Table C to draw the graph.

a. Decide what the independent variable is in the experiment.

b. Decide what the dependent variable is in the experiment.

c. If you need help, read the Procedure, Graphing of Independent and

Dependent Variables.

d. Connect the data points from Trials 1 through 5. Do not draw your line through the data point from Trial 6.

0

100

200

300

400

500

600

0 20 40 60 80 100 120

Volume of HCl (ml)

Vol

ume

H2

gas

(ml)


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3. Analyze the graph in the range of hydrochloric acid volumes between 2 and 50 ml. Question: What is the relationship between the volume of hydrochloric acid added as a reactant and the volume of hydrogen gas (H2) that was produced as a product?

Student answers will vary. For every increase in the volume of

hydrochloric acid, the volume of hydrogen gas increases.

4. Question: In this range of hydrochloric acid volume, do you think that

the hydrochloric acid or the magnesium is greater in amount? Why? (Hint: Remember that you looked into the flask after Trials 1-3 were complete to observe if any magnesium remained.)

Student answers will vary. In this range of hydrochloric acid (HCl)

volume, the magnesium metal (Mg) is in greater amount because

magnesium metal (Mg) was observed to remain after the reactions were

complete.

5. Analyze the graph in the range of hydrochloric acid (HCl) volumes between 50 and 100 ml. Question: What is the relationship between the volume of hydrochloric acid added as a reactant and the volume of hydrogen gas that was produced as a product?

Student answers will vary. For every increase in the volume of

hydrochloric acid used as a reactant, the volume of hydrogen gas

remained the same.

6. Question: In this range of volumes of hydrochloric acid, do you think

that the hydrochloric acid or the magnesium is greater in amount? Why? (Hint: Remember that you looked into the flask after Trials 3-5 were complete to observe if any magnesium remained.) Student answers will vary. In this range of hydrochloric acid volume,

the hydrochloric acid is in greater amount because no magnesium was

observed to remain after the reactions were complete.


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7. Question: If one of the reactants is completely consumed but some of

the second reactant remains unreacted, which reactant limits the amount of products that can be produced? Why?

Student answers will vary. The reactant that is completely consumed

limits the amount of the products that can be produced because there is

no more of that reactant left.

8. Analyze the graph in the range of hydrochloric acid volumes between 50

and 100 ml. Question: Why did the diameter of the balloon and the volume of hydrogen gas remain unchanged in this range of hydrochloric acid volumes?

Student answers will vary. The magnesium was completely consumed

in this range of hydrochloric acid volumes because the hydrochloric

acid was present in a greater amount.

Background Sometimes one reactant is present in a greater amount than the second reactant. The result of such a reaction is that one reactant is completely consumed and a portion of the second reactant remains unreacted. A smaller amount of the products are produced than if both reactants are present at the greater amount. The Law of Conservation of Matter is obeyed even when two reactants are not present in equivalent amounts. In such a reaction, none of the matter is lost even if only a portion of the matter of one reactant remains unreacted.


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9. Analyze the graph for the two data points for the reactions of 0.5g of magnesium and 1g of magnesium metal with 100 ml of hydrochloric acid. Question: Compare the volume of hydrogen produced by the reactions of 0.5g and 1g of magnesium with 100 ml of hydrochloric acid. Which reaction produced a greater volume of hydrogen H2? Student answers will vary. The reaction using 1g of magnesium

produced the greater volume of hydrogen.

10. Question: Why did one reaction produce more hydrogen H2 gas than the

other? Student answers will vary. More hydrogen gas was produced in the

reaction using 1g of magnesium because unreacted hydrochloric acid

remained.

11. Question: In the reaction of 100 ml of hydrochloric acid and 0.5g of

magnesium, which reactant was present in the lesser amount? Explain your answer.

Student answers will vary. The magnesium was present in the lesser

amount because the 0.5g of magnesium was used up. When a greater

amount of magnesium, 1g, was added to 100 ml of hydrochloric acid,

more hydrogen gas was produced suggesting that an excess of

hydrochloric acid remained after the 0.5g of magnesium was used up.

12. Written below is the chemical reaction that you have been studying.

Circle the two products you have observed.

Mg + 2 HCl → MgCl2 + H2 Magnesium

Metal Hydrochloric

Acid Magnesium

Chloride Hydrogen

gas


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Tool: Conclusions At the beginning of the Investigation, you used the Prediction tool to think of possible answers to the following questions. Use the Conclusions tool to answer the questions based on your results from this Investigation. • Are the reactants always completely used up in a chemical reaction?

If the reactants are present in equal amounts, then each reactant will

be completely used up.

• Does the matter making up the reactants disappear?

The matter making up the reactants does not disappear, it is found in

the products of the reaction.

• What happens if there is more of one reactant than the other reactant?

If there is more of one reactant than the other reactant, then it will

not be completely used up in the reaction.

• How do you know when a chemical reaction has stopped?

No more products are produced when a chemical reaction has

stopped.


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Focus Questions: In a chemical reaction, do the amounts of the reactants affect the amounts of products produced? Student answers will vary. Reactants must be present in the reaction in

equivalent amounts to produce the maximum amount of all products.

How does the Law of Conservation of Matter relate to chemical reactions? Student answers will vary. No matter is lost from a chemical reaction even

if the reactants are present in amounts that are not equivalent. Every atom

of every reactant can be found in either the products or in reactants that

are not consumed.


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Chemical Reactions Performance Assessment

Data Record Name: Date:

You are a food chemist who works for the Sweet Tooth Cola Company. You are responsible for testing a chemical reaction that will produce the gas, carbon dioxide, for carbonating the Company’s cola soft drink. The reaction must produce large amounts of carbon dioxide but cannot be very expensive. The chemical reaction that has been used by your co-worker is: The company has decided that one way to reduce the cost of producing the carbon dioxide is by using vinegar instead of pure acetic acid. Vinegar contains acetic acid but is less expensive. Costs can also be reduced by using baking soda which is the chemical sodium bicarbonate. Your co-workers were able to produce some carbon dioxide using the baking soda and vinegar. The different amounts of reactants that your coworkers tried and the volume of carbon dioxide gas they were able to produce are shown in the graph that follows. However, the company still needs to produce carbon dioxide for the soda and also company needs to keep its costs down. They ask you to take over the project. The goals of your project are shown following the graph.

CH3CO2H + NaHCO3 → CO2 + H2O + NaCH3CO2 Water Acetic

Acid Carbon dioxide

Sodium bicarbonate

Sodium acetate


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Goals

1. To keep costs down, design an experiment that produces as large a volume of CO2 gas as possible using as small a mass of sodium bicarbonate as possible. Your experiment should create a larger volume of CO2 gas than that of your co-workers.

2. Explain why you chose the conditions for your experiment. 3. Test your experiment and provide data that shows the results of the

experiment. Your results must include a graph showing your data. 4. Explain whether the volume of carbon dioxide you produced is more than

the carbon dioxide produced by your co-workers and why. 5. Report the volume of vinegar used and the mass of sodium bicarbonate

that you recommend using to produce the largest amount of carbon dioxide at the lowest cost.

6. Explain why your recommendations are the best method for producing

the carbon dioxide at the lowest cost.

Volume of Vinegar (ml)

Vol

ume

of C

O2 g

as (m

l)

0

20

40

60

80

100

120

140

0 5 10 15 20 25 30

Coworker Data Using 1g of baking soda


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Guidelines For Your Experiment

1. To reduce costs you may not use more than 30 ml of vinegar for any one reaction.

2. To reduce costs, you may not use more than 5 grams of baking

soda in any one reaction. 3. You must use the balloon and flask procedure to conduct your

experiment and test the amount of carbon dioxide produced. The procedure is described in the Background.


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Background You will use the same procedure that your coworkers developed to test the reaction. The procedure that was used is shown below: 1. Pour the liquid reactant into a 500ml Erlenmeyer flask. 2. Use a lab scoop to add the solid reactant to a large balloon. 3. Stretch the open end of the balloon over the mouth of

the Erlenmeyer flask until the balloon securely covers the mouth of the flask. Do not allow any solid reactant to fall into the flask.

4. Making sure that the balloon does not come off the

mouth of the flask, hold the balloon and shake the solid reactant out of the balloon until all of it has fallen into the liquid reactant.

5. Gently swirl the flask so the solid reactant stays in contact with the liquid.

After approximately 5 minutes, the production of the product will have stopped. Do not remove the balloon.

6. Use the metric ruler to measure the diameter of the balloon. 7. Calculate the volume of gas produced using the following procedure.

Since the balloon is a sphere, the formula for the volume of a sphere can be used.

In the following equations: π = 3.14 r = the radius of a sphere in centimeters d = the diameter of a sphere in centimeters d3 = (d • d • d)

The volume of a sphere = 4 • π • r3

3 This can be simplified to:

Volume of a sphere = 0.52 • d3 = 0.52 • (d • d • d)


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1. Design an experiment that produces as large a volume of carbon dioxide as possible using the smallest amount of baking soda. The volume of carbon dioxide must be greater than that of your co-workers.

a. Describe the design for your experiment.

To produce the most carbon dioxide, five Trials would be performed.

The Trials would use 30 ml of vinegar but different amounts of

baking soda. The first Trial would use 1 g of baking soda. The

amount of baking soda would be increased to 3 grams in the second

Trial, and increased to 5 grams in the third Trial. The vinegar

would be placed in a flask for each Trial and the baking soda in a

balloon. The balloon would be attached to the flask and the baking

soda added to the flask by holding it above the flask. After each

reaction, the diameter of the balloon would be measured and used to

calculate the volume of carbon dioxide produced.

b. Explain why you chose the conditions for your experiment.

The data from my co-workers showed that they were able to produce

approximately 113ml of CO2 gas. Their graph showed that

increasing the vinegar more than this did not produce a greater

amount of carbon dioxide. This is likely because all of the vinegar

had reacted with the 5 g of baking soda. This indicates that there is

a point in the reaction in which one reactant can be used up even

though there is an excess of another reactant.

The guidelines for the experiment indicate that 30 ml of vinegar

must be used for the experiment. The data from my co-workers

graph shows that 30 ml of vinegar with 1 g of baking soda will not


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produce more carbon dioxide than 10 ml of vinegar. Therefore in

order to increase the amount of carbon dioxide, the amount of

baking soda must need to increase the product of the reaction,

carbon dioxide. However, there is probably a point at which all of

the vinegar in the reaction will react with the baking soda and no

more carbon dioxide will be produced. By increasing the amount of

baking soda in five Trials, I should be able to find that point.

2. Test your experiment and record data from the experiment in the space

below. Your results must include a graph that shows your data.

Reaction

Volume of

Vinegar (ml)

Mass of NaHCO3

(g)

Unreacted NaHCO3

Remaining

Diameter of

Balloon (cm)

Volume of

Balloon (ml)

1 30 1 No 6.0 113 2 30 2 No 7.5 225 3 30 3 No 8.9 375 4 30 4 Yes 8.9 375 5 30 5 Yes 8.9 375

0

50

100

150

200

250

300

350

400

450

0 1 2 3 4 5 6

Vol

ume

of C

arbo

n di

oxid

e (m

l)

Mass of Sodium bicarbonate (g)

Note: All trials used 30ml of vinegar.


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3. Explain whether the volume of carbon dioxide you produced is greater than your co-workers. Support your explanation with data from your experiment.

The volume is greater than the volume produced by the coworkers

based on 375ml of carbon dioxide produced from 3g of sodium

bicarbonate and 30 ml of vinegar. The coworkers produced only 115ml

using 1 of sodium bicarbonate and 10ml of vinegar.

4. Report the volume of vinegar and the mass of baking soda that you

recommend to produce the greatest of carbon dioxide at the lowest cost.

3g of baking soda and 30ml of vinegar produce the greatest amount of

carbon dioxide gas at the lowest cost. Any mass greater than 3 g does

not produce any more gas.

5. Explain why your recommendations are the best method for producing

the carbon dioxide at the lowest cost.

The production of carbon dioxide gas by the coworkers was limited by

using 1g of baking soda and 10ml of vinegar. In my procedure, I

produced more gas because I used 3g of baking soda and 30ml of

vinegar. The increase in the amount of the two reactants increased the

amount of the products.

Background: In a chemical reaction, the chemical bonds that hold the atoms of the reactants together are broken and reformed in a different arrangement to form the products. Breaking and reforming these bonds occurs when the reactants react with each other. The different arrangement of atoms can be seen by the different formulas that represent the reactants and products. When all of the reactants are consumed in a chemical reaction,

Background: In a chemical reaction, the reactants interact to form the products. As the reactants interact, they are consumed at the same time the products are produced. Since the products come from the reactants, the consumption of the reactants takes place at the same rate as the production of products. The rate of a reaction is how much time is required for the complete consumption of the reactants. This is the same amount of time that is required for the productio

chemical reactions idr 10 16 14 - lablearner...10.question: how do you know that a chemical reaction...

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