There are many types of chemical reactions. Four are described below: Synthesis: Two or more reactants combine to form a single product. For example, 2H2 + O2 → 2H2O. (Synthesis reactions are also called combination reactions.)
Decomposition: One reactant breaks down to form two or more products. For example, 2KCl → 2K + Cl2.
Single replacement: An element reacts with a compound to form another element and compound. For example, Zn + 2HCl → ZnCl2 + H2.
Double replacement: Two compounds react to form two different compounds. For example, FeS + 2HCl → FeCl2 + H2S.

Identify the following examples as one of the four choices (from above). In these examples, I’m using letters (A, B, C, D etc) to represent chemical symbols more simply.
Example: X + YZ -> XZ + Y, you would say this is an example of a single replacement reaction.

ABCD -> A + CD + B

AD + CB -> AC + BD

AC + BD -> ACBD

D + EG -> DG + E

Define an Endothermic Reaction:

Define an Exothermic Reaction:

In the following formula, label the Reactants and the Products:
FeS + 2HCl → FeCl2 + H2S



Restate the Law of Conservation of Matter:

Use the Law of conservation of matter to explain what is wrong with the following equation
H2O2 --> H2O + O2 :

pH refers to the acidity of a solution (or alkalinity).
1- 6.9 = Acidic 7= Neutral 7.1 - 14 = Alkaline

Substance pH Acid, Alkaline or Neutral?
Amonia 11 Alkaline

Vinegar 3

Cola 2.5

Water 7

Baking Soda 8

Blood 7.5

Coffee 4