2.1r Chemical Reactions

2026-03-05 22:57

Status: #new

Chemical Reactions

A + $O_{2}$ = AO (Balanced Of Course)
Requires the presence of a $O_{2}$ reactant
Fuel Reactants
- Metal -> Metal Combustion -> Metal Oxide
- Non-metal -> Non-metal Combustion -> Non-metal Oxide
Complete Combustion
- Happens when enough Oxygen Gas is reacted
- All carbons become $C O_{2}$
- $C_{x} H_{y (s)} + O_{2 (g)} \overset{Δ}{\to} C O_{2 (g)} + H_{2} O_{(g)}$
Hydrocarbon or carbohydrate combustion:
- $C H + O_{2} \overset{Δ}{\to} H_{2} O + C O_{2}$
- $C H O + O_{2} \overset{Δ}{\to} H_{2} O + C O_{2}$
Incomplete Combustion
- There is not enough Oxygen Gas to turn all carbons into Carbon Dioxide.
- Thus there is no way to balance
- $C_{x} H_{y (s)} + O_{2 (g)} \overset{Δ}{\to} C_{(s)} + C O_{(g)} + C O_{2 (g)} + H_{2} O_{(g)}$
- Issues with Incomplete Combustion
  - Lower energy efficiency (~ <50% efficiency)
  - Pollution (Carbon $C_{(s)}$ or Soot)
  - Toxicity
    - Carbon Monoxide can fit in the Hemoglobin molecule. This is because of a perfectly designed hole for oxygen gas fits carbon monoxide (LDF). As CO is absorbed into the blood, it gets stuck inside the hemogoblin. With enough exposure, all Hemogoblin cells are filled with CO, which is lethal.

A + B -> AB
Multiple Reactants -> One Product
**Metal Oxide + Water -> Metal Hydroxide
- $C a O_{(s)} + H_{2} O_{(a q)} \to C a (O H)_{2}$
Non-Metal Oxide + Water -> Acid
- $C O_{2 (g)} + H_{2} O_{(l)} \to H_{2} C O_{3 (a q)}$
- Carbon Dioxide + Water -> Carbonic Acid
Metal Element + Non-metal (not oxygen) produces salt (most ionic compounds are salts!)
- $C u_{2} O_{(s)} + H_{2} O_{(g)} \to C u O H_{(s)}$

AB -> A + B
Binary Compound
- $H_{2} O_{(g)} \to H_{2 (g)} + O_{2 (g)}$
- $2 H_{2} 0_{(g)} \overset{e l e c t r i c i t y}{\to} 2 H_{2 (g)} + O_{2 (g)}$ (This is the electrolysis of water)
Base Metal Hydroxides
- $F e (O H)_{2} \overset{Δ}{\to} F e O + H_{2} O$
- Iron Hydroxide -> Iron(II) Oxide + Water
Oxyacids
- Oxyacids are basically always aqueous. Same with binary acids!
- $H_{2} S O_{4 (a q)} \overset{Δ}{\to} S O_{3 (g)} + H_{2} O_{(g)}$
Metal Carbonates
- Basically just solids, unless they are exceptions (Ammonium and Salts of Group 1)
- $C u C O_{3 (s)} \overset{Δ}{\to} C u O_{(s)} + C O_{2 (g)}$

A + BC -> AC + B
Conditions:
- Requires an aqueous environment (at least one aqueous reactant)
Types of Single Displacement
- Metal Displaces the cation and forms a solid salt
- Halogen displaces the halide (check solubility)

AB + CD -> CB + AD
Reaction condition
- Requires at least one aqueous reactant
- There must be at least one product that is not aqueous
If there is no change, state that "both products are aqueous"
Make sure to use your solubility table and guidelines!

**Solid (Precipitate)
- Creates a solid product in aqueous environments
- ie. $F e C l_{2 (a q)} + B a (O H)_{2 (a q)} \to F e (O H)_{2 (s)} + B a C l_{2 (a q)}$
Gas
- Carbon Dioxide Gas
  - $M e t a l C O_{3} + A c i d \to S a l t + H_{2} O_{(s)} + C O_{2 (g)}$
  - $M e t a l H C O_{3} + A c i d \to S a l t + H_{2} O_{(s)} + C O_{2 (g)}$
- Sulphur Dioxide Gas
  - $M e t a l S O_{3} + A c i d \to S a l t + H_{2} O_{(s)} + S O_{2 (g)}$
  - $M e t a l H S O_{3} + A c i d \to S a l t + H_{2} O_{(s)} + S O_{2 (g)}$
- Ammonia Gas
  - $N H_{4} M e t a l + B a s e O H \to S a l t + H_{2} O_{(s)} + N H_{3 (g)}$
- Dihydrogen Sulphide
  - $M e t a l S u l f u r + A c i d \to S a l t + H_{2} S_{(g)}$

Acid + Base -> Salt + $H_{2} O_{(l)}$
Ie. $H_{2} S O_{4 (a q)} + B a (O H)_{2 (a q)} \to B a S O_{4 (s)} + 2 H_{2} O_{(l)}$