Unit 9 - Balancing and Types of Reactions

Balancing

100

Balancing the following: 

 Fe+ Cl₂ →  FeCl₃

2Fe + 3Cl₂ → 2FeCl₃

200

Balance the following: 

HSiCl₃ + H₂O→ H₁₀Si₁₀O₁₅ + HCl

10HSiCl₃ +15H₂O→ H₁₀Si₁₀O₁₅ +30HCl

300

Balance the following:

C₅H₈O₂ + NaH+ HCl → C₅H₁₂O₂ + NaCl

C₅H₈O₂ + 2NaH+ 2HCl → C₅H₁₂O₂ + NaCl 

400

Balance the following:

C₇H₉ + HNO₃ → C₇H₆(NO₂)₃ + H₂O

C₇H₉ + 3HNO₃ → C₇H₆(NO₂)₃ + 3H₂O

500

Balance the following:

CO +  H₂  →  C₈H₁₈ +  H₂O

8CO + 17H₂  → C₈H₁₈ + 8H₂O

Solubility

100

Compounds containing K⁺ are always...

Soluble

200

Compounds containing NO₃^- are always...

Soluble

300

Does the following form a precipitate?

KI + BaS → 

NO RXN

400

What is the precipitate in the following reaction?

NaOH + FeBr₃  → 

Fe(OH)₃

500

What is the full balanced equation for the following reaction with states of matter

BaCl_2(aq) + AgNO_{3(aq)  →} 

BaCl_2(aq) + 2AgNO_{3(aq)  →}  2AgCl_(s) + Ba(NO₃)_2(aq)

Types of Reactions

100

Classify the following: 

Al₂(SO₄)₃ + BaCl₂ → BaSO₄ + AlCl₃

Double replacement

200

Classify the following:

Al₂S₃ → Al + S

Decomposition

300

Classify the following: 

Zn(s) + CuSO₄(aq) → Cu(s) + ZnSO₄(aq)

Single Replacement

400

Classify the following:

H₂ + N₂  → NH₃

Synthesis

500

Classify the following:

CH₄(g)+2O₂(g) → CO₂(g)+2H₂O(g)

Combustion

Activity Series

100

Which metal, when added to hydrochloric acid (HCl), will produce hydrogen gas (H₂)?

A. Zinc (Zn)

B. Gold (Au)

C. Silver (Ag)

A.  Zinc (Zn)

200

A piece of silver metal (Ag) is placed in a solution of zinc nitrate (Zn(NO₃)₂). Will a reaction occur?

No reaction will occur.

Think: Silver (Ag) is below zinc (Zn) on Table J, meaning Ag is less reactive and cannot replace Zn.

300

What type of reaction is the following:

C₂H_6(g) + O_2(g) → CO_{2 (g)} + H₂O_(g)

Combustion

400

Explain why Zn(s) can replace Cu in the following chemical reaction:

Zn(s) + CuSO₄(aq) → Cu(s) + ZnSO₄(aq)

Hint: Explain in terms of activity series

• Zinc (Zn) is a more reactive metal than Copper (Cu) in the activity series.
• When solid zinc is added to a solution of copper(II) sulfate (CuSO₄), zinc replaces copper in the compound, forming zinc sulfate (ZnSO₄) in solution and solid copper as a precipitate.

500

A strip of magnesium metal is placed into a solution of copper (II) sulfate (CuSO₄). Based on Table J, will a reaction occur? Write the balanced chemical equation if a reaction occurs.

Mg(s) + CuSO₄(aq) → Cu(s) + MgSO₄(aq)

Miscellaneous

100

Describe a type of chemical reaction and give an example of one using letters.

Ex. Synthesis 

A + B → AB

200

Why do we balance equations?

To uphold a Conservation of Mass

300

What are always the products for a combustion reaction?

CO₂ and H₂O

400

Compare and contrast an empirical and molecular formula

Empirical = The simplest whole-number ratio of elements in a compound.

Molecular = The actual number of atoms of each element in a molecule of the compound.

500

During a double reaction, one of two things needs to be produced in order for a reaction to occur. What are those two things?

The following needs to be formed:

1. A percipitate

2. A gas