Answer:
1. P
2. A/B
3. A/B
4. R/O
5. P
6. R/O
7. A/B
8. P
9. R/O
10. R/O
Step-by-step explanation:
Precipitation:
Ag (aq) + HCl (aq) → H₂ (g) + AgCl↓
Precipitation reactions can contain a single element.
Certainly, two soluble solutions are mixed, forming an insoluble solid.
Reactions can be identified using a solubility chart, because solubility can affect the precipitacion's equilibrium.
Acid base:
Certainly you mix an acid(H+) an a base (OH-)
We talk about neutralization because we make water. And, there is also a formed salt.
HNO₃ + KOH → H₂O + KNO₃
H⁺ + OH⁻ ⇄ H₂O Kw
Redox:
This is the reaction where moles of electrons are transferred and gained.
A pure element is consumed or formed. We have 2 half reactions:
- Reduction (oxidation state decreases, electrons are released)
- Oxidation (oxidation state increases, electrons are gaines)
Reactions involving pure O₂ are named combustion, which is a redox type.
This is an example of redox decomposition of hydrogen peroxyde.
2H⁺ + H₂O₂ + 2e⁻ → 2H₂O
H₂O₂ → 2H⁺ + O₂ + 2e⁻
H₂O₂ → 2H₂O + O₂