Chemical Reactions

Energy of Reactions

For each of the following graphs, indicate the following:a) Determine the H of each reaction. Show work.b) Is the reaction exothermic or endothermic?c) Does it require activation energy? How much? Show work.d) What is the net result of the change in heat energy? (Temperature does what?)

80

60

40

20

En

er gy

kJ

50

40

30

20E

ner gy

kJ

30

20

10

0

En

er gy

kJ

Course of reaction Course of reactionCourse of reaction

3.

2.

1.

12 energy graphs to analyze

Drawing Energy of Reaction Graphs

For each of the following examples, draw the appropriate corresponding graph of energy of the reaction.

a)Make sure to label both axesb)Label the H of each reaction. c)Label the activation energy, if needed.

1. Exothermic reaction with activation energy 2. Endothermic reaction with activation energy

4. Temperature is increased with use of activation energy.3. Absorbs energy from surroundings with activation energy.

10 energy drawings

80

70

60

50

En

er gy

kJ

45

35

25

15

En

er gy

kJ

Course of reaction Course of reaction

1.

2.

3.

Course of reaction

100

50

0

-50

En

er gy

kJ

Quiz-Energy of Reactions

For each of the following graphs, indicate the following:

a) Determine the H of each reaction. Show work.b) Is the reaction exothermic or endothermic?c) Does it require activation energy? How much? Show work.d) What is the net result of the change in heat energy? (Temperature does what?)

Quiz-Endothermic/Exothermic

An ice pack is used in athletic events when a player has an injury. An ice pack contains two different chemicals that when combined together cause a chemical reaction to happen. This reaction is responsible for the sudden decrease temperature of the pack. Draw an energy diagram of this reaction. On your diagram, label the H and activation energy. Is this reaction endothermic or exothermic? Describe the net result change in energy (temperature).

Names and Formula Practice

Write names and/or formulas for each compound.

1. Cl5O5 ________________________2. C3S6 ________________________3. MgCl2 ________________________4. Si3F6 ________________________5. AsSe2 ________________________6. NO2 ________________________7. Al(NO3)3 _______________________8. Zn(ClO3)2 ________________________9. S4O8 ________________________19. Al2S3 ________________________20. Si2O4 ________________________

21. dicarbon tetrachloride _____________22. trichlorine pentacarbon _____________23. phosphorus mononitride _____________24. dinitrogen hexoxide _____________25. tetraphosphorus dioxide _____________26. selenium dioxide _____________27. strontium bromide _____________28. carbon trisulfide _____________29. phosphorus triiodide _____________30. diselenium trioxide _____________31. barium nitride _____________32. tritellurium dinitride _____________

60 names and formulas to write; mixed ionic and covalent

Write names and formulas for

each compound.

aluminum iron II copper I ammonium calcium

chlorine1. 2. 3. 4. 5.

sulfate6. 7. 8. 9. 10.

phosphate11. 12. 13. 14. 15.

chlorate16. 17. 18. 19. 20.

hydroxide21. 22. 23. 24. 25.

chromate26. 27. 28. 29. 30.

oxygen31. 32. 33. 34. 35.

permanganate36. 37. 38. 39. 40.

phosphorus41. 42. 43. 44. 45.

60 ionic formulas to write

Introduction to Equations

Read each statement. Write the correct formula for the substance indicated. Replace each “and” or “plus” with the symbol “+”.

Replace each “produces” or “make” with an arrow pointing toward the right. Count total number of atoms of each substance on each side of the arrow. (see example)

Example:Lead II nitrate and potassium carbonate produce lead II carbonate and potassium nitrate.Pb(NO3)2 + K2CO3 PbCO3 + KNO3

Pb-1 Pb-1N-2 N-1O-9 O-6K-2 K-1C-1 C-1

1. aluminum and oxygen make aluminum oxide

2. sodium hydroxide and hydrogen sulfate produce sodium sulfate and hydrogen hydroxide

3. iron and copper II chloride make iron II chloride and copper

4. potassium chlorate produces potassium chloride and oxygen

20 equations to write and count

Balancing Equations Worksheet

Use coefficients to balance each equation. Formulas are written correctly.

1. Ag3PO4 + KBr K3PO4 + AgBr

2. H2SO4 + O2 H2SO4

3. ZnS + O2 ZnO + SO2

4. Na2SO4 + Fe(NO3)3 NaNO3 + Fe2(SO4)3

5. AgNO3 + CaCl2 AgCl +Ca(NO3)2

6. Al2O3 + HCl AlCl3 + H2O

20 equations to balance

Quiz-Introduction to Equations

Write a balanced equation for the following.

1. calcium phosphate and hydrogen carbonate make calcium carbonate and hydrogen phosphate

2. iron and oxygen produce iron III oxide

Word Equations Write a balanced equation to represent each of the following chemical reactions.

1. iron (III) and lead IV sulfide

2. aluminum hydroxide and potassium dichromate

3. silver and magnesium bromide

4. fluorine and aluminum chloride

5. sodium and tin (IV) nitrate

6. aluminum sulfate and magnesium

15 equations to predict and write

What is the generic form of each?

Type of reaction?

How are these alike?

What do you look for that tells you the type of reaction?

What steps do you follow to write a balanced equation?

Chemical Reactions

Quiz-Predicting, Balancing and Types

Write a balanced equation and indicate the type of reaction in the blank beside each set of reactants.

_____ 1. potassium + nitrogen

_____ 2. C2H6 + oxygen

_____ 3. strontium chloride

_____ 4. calcium acetate + aluminum carbonate

_____ 5. zinc bromide + chlorine

Assigning Oxidation Numbers:

Assign oxidation numbers to all of the elements in each of the compounds or ions below.

1. HCl

2. KNO3

3. OH-

4. KClO3

5. Al(NO3)3

6. PbO2

7. NaHSO4

8. H2SO3

24 formulas to assign oxidation numbers

Redox Reactions:For the equations below, identify the oxidation number of each

species that changes oxidation number, the substance oxidized and the substance reduced and the oxidizing agent and reducing agent.

1. H2 + O2 H2O

2. Fe + ZnCl2 FeCl3 + Zn

3. Al + Fe(NO3)2 Al(NO3)3 + Fe

4. Cu + AgNO3 Cu(NO3)2 + Ag

5. Al + Br2 AlBr3

6. Al + Fe2O3 Al2O3 + Fe

7. HNO3 + H2S S + NO + H2O

12 redox equations to analyze

Redox Reactions-Equations to BalanceBalance the following equations. Write oxidation numbers; half-reactions;

balanced redox equation. Identify substance oxidized and substance reduced.

1. Cu + AgNO3 Ag + Cu(NO3)2

2. CdS + I2 + HCl CdCl2 + HI + S

3. NaClO + H2S NaCl + H2 SO4

4. CaCl2O + NaAsO2 + NaOH CaCl2 + Na3AsO4 + H2O

5. KBr + Fe2(SO4)3 Br2 + K2SO4 + FeSO4

16 redox equations

Quiz-Redox

Write a balanced molecular equation.Assign oxidation numbers; write the half-reactions and the resulting equation.Identify the substance oxidized and the substance reduced.

1. nickel (II) oxide

2. zinc + copper (I) chloride

Volt- meter

Ag

wire

Cd

1 M AgNO ,100 milliliters

1 M Cd(NO ) ,100 milliliters

saltbridge

3 2 3

Ag Cu

Electrochemistry Cells

Write the half-reactions for each equation.Determine which substance is oxidized and which is reduced.Write a balanced redox equation.

Label the drawing: AnodeCathodeDirection of electron flowSolution in each beaker

1. Cu + AgNO3 Ag + Cu(NO3)2

5 electrochemistry cells to label and write equations for

#4

Complete and balance these combustion reactions.

1. C2H6

2. C7H16

3. C5H12

4. C10H22

Review

8 Horse Race

Cards

Use the answer choices below for questions 5-8. No answer will be used more than once.

A. CS2 + 3 O2 CO2 + 2 SO2

B. Zn + NiCl2 Ni + ZnCl2 C. CaO + SO2 CaSO3

D. 3 PbOH2 + 2 H3PO4 Pb3(PO4)2 + 6 HOHE. C3H7OH + 5 O2 3 CO2 + 4 H2O

_____5. A single replacement reaction_____6. An equation that is incorrectly balanced_____7. An equation containing formulas that are written incorrectly_____8. An equation which an oxidation number changes from -2 to +4

_____2. A 5.0 gram sample of magnesium and a 50 mL sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the slowest reaction rate?

a) a magnesium strip and 1.0 M HCl b) a magnesium strip and 3.0 M HClc) magnesium powder and 1.0 M HCld) magnesium powder and 3.0 M HCl

Test over Chemical Reactions

25 questions

Test over Chemical Reactions

25 questions

20. When the equation below is correctly balanced, the sum of the coefficients is

zinc chlorate and iron III nitrite

a) 4b) 8c) 10d) 12e) 20

Identify the type of reaction and write a balanced equation._________4. sodium carbonate + calcium hydroxide

_____16. Based on the graph to the left, the ∆H of the reaction is

a. 60 kJ c. 80 kJb. – 60 kJ d. -80 kJ

_____17. The amount of activation energy needed when a catalyst is present is

a. 60 kJ c. 140 kJb. 100 kJ d. 20 kJ

Chemical Reactions Test continued