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Lab 4 Reaction Products Worksheet Section 1: Identify the type of reaction For the following reactions, indicate whether the following are examples of synthesis, decomposition, combustion, single displacement, or double displacement:

1)

Na3PO4 + 3 KOH  3 NaOH + K3PO4 - DOUBLE DISPLACEMENT

2)

MgCl2 + Li2CO3  MgCO3 + 2 LiCl - DOUBLE DISPLACEMENT

3)

C6H12 + 9 O2  6 CO2 + 6 H2O - COMBUSTION

4)

Pb + FeSO4  PbSO4 + Fe - SINGLE DISPLACEMENT

5)

CaCO3  CaO + CO2 - DECOMPOSITION

6)

P4 + 3 O2  2 P2O3 - SYNTHESIS

7)

2 RbNO3 + BeF2  Be(NO3)2 + 2 RbF - DOUBLE DISPLACEMENT

8)

2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag - SINGLE DISPLACEMENT

9)

C3H6O + 4 O2  3 CO2 + 3 H2O - COMBUSTION

10)

2 C5H5 + Fe  Fe(C5H5)2 - SYNTHESIS

11)

SeCl6 + O2  SeO2 + 3Cl2 - SINGLE DISPLACEMENT

12)

2 MgI2 + Mn(SO3)2  2 MgSO3 + MnI4 - DOUBLE DISPLACEMENT

13)

O3  O. + O2 - DECOMPOSITION

14)

2 NO2  2 O2 + N2 - DECOMPOSITION

Section 2: Practicing equation balancing

Before you can write a balanced equation for a problem which asks you to predict the products of a reaction, you need to know how to balance an equation. Because some of you may not fully remember how to balance an equation, here are some practice problems:

1)

2C6H6 +15 O2 6H2O +12CO2

2)

4NaI +1Pb(SO4)2 1 PbI4 +2 Na2SO4

3)

2H3 +2O2 1NO +3H2O

4)

2Fe(OH)3  1 Fe2O3 + 3 H2O

5)

2HNO3 +1 Mg(OH)2 2H2O +1Mg(NO3)2

6)

1H3PO4 +3NaBr 3HBr +1Na3PO4

7)

3C +4H2 1C3H8

8)

2CaO +1MnI4 1MnO2 +2CaI2

9)

1Fe2O3 +3H2O 2Fe(OH)3

10)

1C2H2 +2H2 1C2H6

11)

2VF5 +10HI 1V2I10 +10HF

12)

1OsO4 +2PtCl4 2PtO2 +1OsCl8

13)

1CF4 +2Br2 1CBr4 +2F2

14)

2Hg2I2 +1O2 2Hg2O +2I2

15)

1Y(NO3)2 +1GaPO4 1YPO4 +1Ga(NO3)2

Section 3: Predicting the products of chemical reactions Predict the products of the following reactions:

1)

2Ag + 1CuSO4 1Ag2SO4 + 1Cu

Type: Single Displacement 2)

2NaI + 1CaCl2 2NaCl + 1Cal2

Type: Double Displacement 3)

1O2 + 1H2  2H2O

Type: Synthesis 4)

2HNO3 + 1Mn(OH)2  2H2O + 1Mn(NO3)2

Type: Acid-Base

5)

2AgNO2 + 1BaSO4  1Ag2SO4 + 1Ba(NO2)2

Type: Double Displacement 6)

2HCN + 1CuSO4  1H2SO4 + 1Cu(CN)2

Type: Double Displacement 7)

1H2O + 1AgI  1HI + 1AgOH

Type: Double Displacement 8)

3HNO3 + 1Fe(OH)3  3H2O + 1Fe(NO3)3

Type: Acid-Base 9)

4LiBr + 1Co(SO3)2  2Li2SO3 + 1 CoBr4

Type: Double Displacement 10)

1LiNO3 + 1Ag  1AgNO3 + 1Li

Type: Single Displacement 11)

1N2 + 2O2  2NO2

Type: Synthesis 12)

1H2CO3  1CO2 + 1 H2O

Type: Decomposition 13)

1AlCl3 + 3 Cs  3CsCl + 1Al

Type: Single Displacement 14)

1Al(NO3)3 + 1Ga  1Ga(NO3)3 + 1Al

Type: Single Displacement 15)

1H2SO4 + 2NH4OH  2H2O + 1(NH4)2SO4

Type: Acid-Base

Write the letter of the correct match next to each problem. a. Double displacement 1. (metathesis)

Two reactants result in single product. Ans – f

b. One reactant that results in multiple products. 2. Balanced Equation

Ans - q c. Gas formation usually seen as bubbles in solution.

3. g

Ans - h d. Appearance of a solid when two solutions are mixed..

4. physical change

Ans - l e. Solid

5. heat content change

Ans - s f. An exchange of elements (partners) between two compounds.

6. Products

Ans - k g. The chemicals the reaction starts with.

7. Exothermic

Ans - m h. Gas

8. combination reaction

Ans - a i.

9. Color change

Symbolic representation of chemical reactions. Ans – c

j. 10. decomposition

Liquid Ans – b

k. The chemicals the reaction ends with. 11. Endothermic

Ans – o l.

12. s 13. aq

A change that does not effect the chemical composition of an element or compound. Ans – e

m. Reaction releases energy.

Ans – r n. One element in a compound is replaced by another. 14. l

Ans – j o. Reaction absorbs energy.

15. Chemical Equation

Ans – i p. Carbon and hydrogen containing compounds combine with oxygen and heat to produce carbon dioxide and water.

Single substitution 16. reaction

Ans – n q. Elements on both sides of equation are equal.

17. Reactants

Ans – g r.

18. Precipitate formation

Aqueous Ans – d

s. Temperature increase or decreases. 19. Combustion reaction

Ans – p...