Module 5i Homework Packet

CHM 1025C Name: _________________

Module Five I Homework Packet-Hein

Module 5i: Chemical Equations & Stoichiometry (Chapter 8)

E._____(02) Writing Reactions/ Symbols-Section 8.1 Answers

E1.____(02) Classifying Chemical Reactions- Section 8.3 Answers

F._____(05) Balancing Chemical Equations -Sections 8.2 Answers ef

G._____(04) Predicting Single Replacement Products . Sections 8.3 Answers

H._____(04) Predict Double Replacement Sections 8.3 Answers h

H1____ (04) Neutralization/Gas Forming Reactions 15.6 ,Lecture Answers

______(21) Module 5i Total (Ninth Exam)

Foundations of College Chemistry, 14th Edition

Table of Contents
Chapter 8 Chemical Equations 143

8.1 The Chemical Equation 144

8.2 Writing and Balancing Chemical Equations 145

8.3 Types of Chemical Equations 150

8.4 Heat in Chemical Reactions 156

8.5 Global Warming: The Greenhouse Effect 159

Review 161

Review Questions, Paired Exercises 163

Additional Exercises 165

Challenge Exercise, Answers to Practice Exercises 166

In Module Three we studied the composition of an atom.

In Module Four we made compounds.

In Module Five we finally should be able to react

these compounds in chemical reactions.

(or summarize a chemical change we studied in Module 1).

From Your Hein Textbook and Power Point for Chapter 8, what is a chemical equation?

Evidence for Chemical Reactions

There are four observations that indicate a chemical reaction is taking place:

1. A gas is produced.

Gas may be observed in many ways in a reaction from light fizzing to heavy bubbling.

2. An insoluble solid is produced in a solution.

a. A substance dissolves in water to give an aqueous solution.

b. If we add two aqueous solutions together, we may observe the production of a solid substance.

c. The insoluble solid formed is called a precipitate

3. A permanent color change is observed.

a. Many chemical reactions involve a permanent color change.

b. A change in color indicates that a new substance has been formed

4. An energy change is observed

a. A reaction that releases heat is an exothermic reaction.

b. A reaction that absorbs heat is an endothermic reaction.

c. Examples of a heat energy change in a chemical reaction are heat and light being given off.

From the Corwin Textbook, the Chemical symbols are explained:

M-5i Homework Packet

Module Five-Part E Basic Stoichiometry Definitions 2 points

Fill in the following with the symbols used in chemical equations which has the stated translation or meaning(s) (Corwin Section 7.2 Table 7.1 page 191 Corwin 7^th ) (Hein Section 8,1 Table 8.1 page 144):

_________1. Produces, yields, gives

_________2. Reacts with, added to, plus

_________ and _________ 3. Solid substance or precipitate forms

_________and _________4. Gaseous substance formed

_________5. Liquid Substance

________5a. Water or aqueous solution

_________6. Reversible Reaction

_________7. No Reaction

8. Show the symbol for heat:__________

9. How would you show a catalyst in a chemical reaction where A plus B forms products D and E, but is catalyzed by substance C

A + B à D + E

10. Define Catalyst (See Section 7.2 page 191)

M-5i Homework Packet

In Corwin’s 6^th Section 8.4 five types of reactions: Combination, Decomposition, Single Replacement, Double Replacement, and Neutralization reactions are introduced. The table 8.3 is a summary. Hein Section 8.3 explains the five types.

In Hein’s 14^th edition Section 8.3 is devoted to types of chemical reactions, pages 150-156 which summaried in Chapter 8 Power Point:

From my lecture, I have told you a chemical change via a chemical reaction is either a NON-REDOX or a REDOX change. Combination, Decomposition, Single Replacement and Oxidation-Reduction (more complicated) are REDOX changes. Only Double Replacement, Double Displacement or sometimes called Metatarsus reactions are NON-REDOX and I like to call them Ion-Exchange Reactions,.

Our Hein textbook describes several types of Double Displacement Reactions including gas formation. Our Corwin textbook should have a section 7.12 which is the third type of double replacement (Metatarsus or Ion Exchange):

Gas Forming Reactions.

When predicting the products of a double replacement reaction, sometimes one of the products instantly decomposes.

If H₂CO₃ is a predicted product in ion exchange, it is written as

CO₂ and H₂O.

For example:

Na₂CO₃ (aq) + HCl (aq) à [H₂CO₃](aq) + NaCl (aq)

Should be written:

Na₂CO₃ (aq) + HCl (aq) à CO₂(g) + H₂O (l) + NaCl (aq)

Two other products which are shown differently:

[NH₄OH] à NH₃ + H₂O

[H₂SO₃] à SO₂ + H₂O

In Corwin’s chapter 19 and Hein’s Chapter 20, there is a another type of chemical reaction:

Combustion – a substance burns in the presence of oxygen. Combustion of a compound that contains C and H (or C, H, and O) produces carbon dioxide gas and water.

CH₂O(l) + O₂(g) → CO₂(g) + H₂O(l)

The general type of combustion problem looks like this:

C_xH_y [(l) or (g)] + O₂ (g) à CO₂(g) + H₂O (g)

C_xH_yO_z[(s) or (l) or (g)] + O₂ (g) à CO₂(g) + H₂O (g)

The chemical reaction for the combustion of gasoline:

C₈H₁₈ (l) + O₂ (g) à CO₂(g) + H₂O (g)

Octane oxygen gas carbon dioxide water

Module 5 E1: Classification of Chemical Reactions 2 Points

(Sections 7.4)

Classify Each of the following (unbalanced) chemical reactions as:

Combination (or synthesis)
Decomposition (or Anaylsis)
Single Replacement
Double Replacement (Precipitation)
Double Replacement (Neutralization)
Double Replacement (Gas Forming)
Combustion of a hydrocarbon

______1. Fe + FeCl₃ à FeCl₂

____2_.HCl + Mg(OH)₂ à MgCl₂ + HOH

_____3. Mg + HNO₃ à Mg(NO₃)₂ + H₂

_____4. H₂ + N₂ à NH₃

____5. NaHCO₃ + HCl à NaCl + CO₂ + H₂O

____6. Ca(NO₃)₂ + K₃PO₄ à Ca₃(PO₄)₂ + KNO₃

____7. KClO₃ à KCl + O₂

____8. Na + H₂O à NaOH + H₂

(See Corwin’s Questions #21-24 p215 for more practice) (Hein has no additional practice at the end of the chapter)

Writing Chemical Reactions (Section 7.2)

9. Write a chemical equation for solid cadmium hydrogen carbonate decomposing to yield solid cadmium carbonate, water, and carbon dioxide gas:

10. Write a chemical equation for the reaction of aqueous solutions of potassium chromate and calcium sulfate to give the precipitate calcium chromate and aqueous potassium sulfate.

See additional Corwin’s questions #7-17 p215;

Hein Questions #9-#12 page 164.

Writing Chemical Reactions

11. Write a chemical equation or solid sodium hydrogen carbonate decomposing to yield solid cadmium carbonate, water, and carbon dioxide gas:

12. Write a chemical equation for the reaction of aqueous solutions of potassium chromate and lead(II) nitrate to give the precipitate lead(II) chromate and aqueous potassium nitrate.

Rules and Suggestions for Balancing Equations

1) The same # and type of atom must be present on each side of the equation.

2) Balancing is accomplished by adding coefficients. NEVER change the subscripts.

3) Coefficients must be in the smallest whole # ratio.

4) Balancing is done by trial and error.

5) Usually Balance H’s and O’s last or an element that appears in more than one place of either side of the reaction .

6) Balance polyatomic ions as one unit in Ion Exchange reactions.

M-5i Homework Packet

Example of balancing an Equation:

Module Five-Part F Balancing Chemical Equations 5 points

Balance the following chemical equations (write the chemical formulas in #10 then balance):

1. Fe + FeCl₃ à FeCl₂

2. Al + O₂ à Al₂O₃

3. Na₂CO₃ + C + N₂ à NaCN + CO

4. FeS + O₂ à Fe₂O₃ + SO₂

5. IBr + NH₃ à NI₃ + NH₄Br

6. Cl₂ + HOH à HCl + HClO

7. AgNO₃ à AgNO₂ + O₂

8. HClO₄ + P₄O₁₀ à H₃PO₄ + Cl₂O₇

9. HCl + Mg(OH)₂ à MgCl₂ + HOH

10. Sodium hydroxide + Hydrochloric acid à sodium chloride + water

Hein Additional Practice: Page 163 Questions #3-#8

You may check your work using the online chemical equation balancer at:

http://people.emich.edu/bramsay1/ccc-release/chem.html

Video:
https://www.khanacademy.org/test-prep/mcat/physical-processes/stoichiometry/v/balancing-chemical-equations

M-5i Homework Packet

See Sections 7.7 and 7.8. Extra practice questions on page 216 #47-52; and #53-55 page 217.

M-5i Homework Packet

If you were to (H₂O) in the activity series like an acid is shown as (H), where would you put it? Show below:

Given the following Activity Series:

Li > K > Ba > Sr > Ca > Na > Mg > Al >

Mn > Zn > Fe > Cd > Co > Ni > Sn >

Pb > (H) > Cu > Ag > Hg > Au

The rule to follow is a single replacement reaction takes place only if the metal or (H) is more active than the metal or (H) it is replacing. Li will react with everything, while Hg will replace only gold. And poor gold does not react with any of the cations of metals. Therefore gold is found pure in nature, while the very active metals such as potassium and sodium are never found pure in nature, but are found as minerals (ionic compounds).

Will Mg metal react with Nitric Acid? Yes
(Mg has a great reactivity then [H] in the series)

Mg (s) + 2 HNO₃ (aq) → Mg(NO₃)₂ (aq) + H₂ (g)

Will Copper react with Nitric Acid? no
(Cu is below [H] in the activity series)

Cu (s) + HNO₃ (aq) → no reaction

Given the following Active Metals:

Li > K > Ba > Sr > Ca > Na> (H₂O)

The six very active metals are so reactive they will replace one of the two hydrogens in water and form alkaline hydroxides as products. Hydrogen gas will bubble out of the solution. See some of the above movies for demonstrations.

Will Sodium react with water? yes
(Na is one of the six active metals above)

2 Na(s) + 2 HOH (l) → 2 NaOH (aq) + H₂ (g)

M-5i Homework Packet

Part G Single Replacement Reactions 4 points

Given the following Activity Series:

Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni >

Sn > Pb > (H) > Cu > Ag > Hg > Au

Given the following Active Metals:

Li > K > Ba > Sr > Ca > Na

Complete the products of the following reactions, then balance the equation (If no reaction write NR):

1. Cu (s) + Al(NO₃)₃ (aq) à

2. Al (s) + Cu(NO₃)₂ (aq) à

3. Au (s) + H₂SO₄ (aq) à

4. Ca (s) + H₂O (l) à

5. Mn (s) + H₂O (l) à

For additional Practice:
Hein page 164 Questions #13-#16

M-5i Homework Packet

Except in neutralization and gas forming reactions.

Part H Double Replacement Reactions 4 points

Given the following Solubility Rules for Ionic Compounds:

Compounds containing the following ions are generally soluble in water:

1. Alkali metal ions and ammonium ions, Li⁺ , Na⁺ , K⁺ , NH₄⁺

2. Acetate ion, C₂H₃O₂^-

3. Nitrate ion, NO₃^-

4. Halide ions (X), Cl^- , Br^- , I^- (AgX, Hg₂X₂ , and PbX₂ are insoluble exceptions)

5. Sulfate ion, SO₄^2- (SrSO₄, BaSO₄ , and PbSO₄ are insoluble exceptions)

Compounds containing the following ions are generally insoluble in water:

6. Carbonate ion,CO₃²^- (see rule 1 exceptions which are soluble)

7. Chromate ion CrO₄^2- (see rule 1 exceptions which are soluble)

8. Phosphate ion PO₄^3- (see rule 1 exceptions which are soluble)

9. Sulfide ion, S^2- (CaS, SrS, BaS, and rule 1 exceptions are soluble in water)

10. Hydroxide ion, OH^- [ Ca(OH)₂ , Sr(OH)₂ , Ba(OH)₂ , and rule 1 exceptions are soluble)

Complete and balance the following reactions using the above solubility table (write no reaction or NR if both products are soluble or a covalent compounds is not formed)

1. AlCl₃ (aq) + K₂CO₃ (aq) à