CHM 2045C Name: _________________

Module 5i Homework Packet-Jespersen 7^th

Module Five Part I:Chemical Equations & Stoichiometry (Chap 3-4)

E._____(03) Basic Reaction Symbols-Chapter 3 Section 3.1 Answers ef

E1.____(02) Classifying Chemical Reactions- Section 3.1-Lecture

F._____(05) Balancing Chemical Equations -Sections 3.1 Answers ef

G._____(05) Predicting Single Replacement Products Sections 4.8 Answers

H._____(05) Predict Double Replacement Sections 4.1, 4.3, 4.5 Answers h

H1____ (05) Neutralization/Gas Forming Reactions Section 3.8-3.9-4.5 Lecture Answers

______(25) Total = ______%

M-5i Required Homework:

______(30) M-5i Pretest Hardcopy Homework Packet

______(30) M-5i Multiple Choice (MC) Homework/Exam (Blackboard Online)

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.

Module Five-Part E Basic Stoichiometry Definitions 3 points

CHM 2045C Module Five I Homework Packet

Module Five-Part E Basic Stoichiometry Definitions 3 points

Fill in the following with the symbols used in chemical equations which has the stated translation or meaning(s) :

_________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)

Reference:

Jespersen 7^th Chapter 3 Section 3.1

M-5i Homework Packet

Module 5 E1: Classification of Chemical Reactions 2 Points

(Sections 3.1)

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

1. Combination (or synthesis)
2. Decomposition (or Anaylsis)
3. Single Replacement
4. Double Replacement (Precipitation)
5. Double Replacement (Neutralization)
6. Double Replacement (Gas Forming)

______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

M-5i Homework Packet

Reference:

Jespersen 7^th Chapter 3 Section 3.1

Writing Chemical Reactions (Section 3.1) 1 point

9. Write a chemical equation or 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.

M-5i Homework Packet

Reference: McMurry: Section 3.1

Module Five-Part F Balancing Chemical Equations 5 points

M-5i Homework Packet

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

Reference:

Jespersen 7^th Chapter 3 Section 3.1

M-5i Homework Packet

Module Five-Part F Balancing Chemical Equations

M-5i Homework Packet

Module Five-Part F Balancing Chemical Equations Continued

Reference: McMurry: Chapter 3 Section 3.1

You may check your work using the online chemical equation balancer at: http://people.emich.edu/bramsay1/ccc-release/chem.html

Reference:

Jespersen 7^th Chapter 3 Section 3.1

M-5i Homework Packet

Part G Single Replacement Reactions 5 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

M-5i Homework Packet

Part G Single Replacement Reactions

M-5i Homework Packet

Part G Single Replacement Reactions

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

M-5i Homework Packet

Part G Single Replacement Reactions 5 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

Reference:
Jespersen 7^th Sections 4.8

M-5i Homework Packet

Part H Double Replacement Reactions 5 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,CO₃^2- (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

2. NiSO₄ (aq) + Li₃PO₄ (aq) à

3. NaCl (aq) + AgNO₃ (aq) à

4. H₂SO₄ (aq) + NaOH (aq) à

5. H₃PO₄ (aq) + Ba(OH)₂ (aq) à

Reference:
Jespersen 7^th: Sections 4.1, 4.3, 4.5

M-5i Homework Packet

Part H1 Double Replacement Reaction:

Neutralization/Gas Forming Reactions 5 points

Complete and balance the following precipitation reactions using the above solubility table

(write no reaction if both products are soluble or a covalent compounds is not formed)

1. Mg(OH)₂ (s) + H₂SO₄ (aq) à

2. H₃PO₄ (aq) + KOH (aq) à

3. NH₄NO₃ (aq) + Ba(OH)₂ (aq) à

4. HBr (aq) + Pb(CO₃)₂ (aq) à

5. LiOH (aq) + H₃PO₄ (aq) à

6. Na₂CO₃ (aq) + HCl (aq) à

Note for M-5H1:
Neutralization ion Exchange Reaction:

1. When an acid reacts with a base, salt plus water are the products

Gas Forming Ion Exchange Reactions:

2. When either H₂SO₃; H₂CO₃ or NH₄OH is formed as a product it immediately

decomposes thus demonstrating a gas forming reaction.

3. Most books do not show either H₂CO₃ or NH₄OH as products, just the

decomposed products of the gases and water in the answer.

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

Reference:

McMurry: Section 3.1;

Jespersen 7^th: Chapters 3 & 4Sections 3.8-3.9-4.5