Question

Chemical equations serve a variety of purposes, but the most general form of a chemical equation is reactants -> products. Most often, reactants and products are described by their chemical formula, possibly including a designation of state of matter. Contrary to a general chemical equation, a balanced chemical equation always uses molecular formulas and is amended by stoichiometric factors to assure conservation of mass and/or moles.

Chemical equations represent chemical reactions, and chemical reactions can be classified according to two groups:

Group I (bond breakage and/or bond formation): The four reaction types are Synthesis, Decomposition, Single Displacement, Double Displacement.

Group II (common reaction principles): Representative examples are Precipitation, Redox, Acid-Base, Combustion. Choose from the following general chemical equations, and illustrate the four principle group I reaction types, and the four representative group II reaction types:

A) aqueous potassium sulfate + aqueous barium nitrate -> aqueous potassium nitrate + solid barium sulfate

B) magnesium metal + nitrogen gas -> solid magnesium nitride

C) copper metal + aqueous silver nitrate -> aqueous copper nitrate + silver metal

D) chlorine gas + fluorine gas -> chlorine monofluoride gas

E) aqueous hydrochloric acid + aqueous calcium hydroxide -> aqueous calcium chloride + water

F) gaseous sulfur dioxide + oxygen gas -> gaseous sulfur trioxide

G) solid calcium carbonate -> solid calcium oxide + gaseous carbon dioxide

H) solid silver oxide -> oxygen gas + silver metal

When you discuss reaction types, formulate the chosen general equation as balanced chemical equation.

Any given equation might serve as an example for a group I as well as for a group II reaction, but try to use as many different equations as possible.

Answer 1

Group 1:

A) Double Displacement. (in which two ions gets exchanges)
aqueous potassium sulfate + aqueous barium nitrate -> aqueous potassium nitrate + solid barium sulfate

B) Synthesis ( formation of compound from its elements)

magnesium metal + nitrogen gas -> solid magnesium nitride

C) single Displacement. (in which one ions exchanges with another one)

copper metal + aqueous silver nitrate -> aqueous copper nitrate + silver metal

D) Synthesis ( formation of compound from its elements)

chlorine gas + fluorine gas -> chlorine monofluoride gas

G)decomposition

solid calcium carbonate -> solid calcium oxide + gaseous carbon dioxide

H) decomposition solid silver oxide -> oxygen gas + silver metal

group 2:

A) Precipitation,

aqueous potassium sulfate + aqueous barium nitrate -> aqueous potassium nitrate + solid barium sulfate

B) Redox ( reaction which is having both reduction,oxidation parts)

magnesium metal + nitrogen gas -> solid magnesium nitride

D) Redox ( reaction which is having both reduction,oxidation parts)

chlorine gas + fluorine gas -> chlorine monofluoride gas

E) Acid-Base

aqueous hydrochloric acid + aqueous calcium hydroxide -> aqueous calcium chloride + water

F) combustion gas

gaseous sulfur dioxide + oxygen gas -> gaseous sulfur trioxide

H) Redox    solid silver oxide -> oxygen gas + silver metal