Chemistry, 30.07.2019 18:00, Jwhite8602

Nacl(aq)+hg2(c2h3o2)2(aq)→ express your answer as a chemical equation. enter noreaction if no reaction occurs. identify all of the phases in your answer. nac2h3o2(aq)+hg2cl2(s)nac2h3o2(aq)+ hg2cl2(s)

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The chemical reaction between NaCl and ${\text{H}}{{\text{g}}_{\text{2}}}{\left( {{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_{\text{2}}}} \right)_2}$ is as follows:

$\boxed{{\text{NaCl}}\left( {aq} \right) + {\text{H}}{{\text{g}}_{\text{2}}}{{\left( {{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_{\text{2}}}} \right)}_2}\left( {aq} \right) \to {\text{H}}{{\text{g}}_{\text{2}}}{\text{C}}{{\text{l}}_2}\left( s \right) + 2{\text{Na}}{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_2}\left( {aq} \right)}$

Further explanation:

The five types of chemical reactions are as follows:

1. Combination reactions:

These reactions are also known as a synthesis reaction. These are the reaction in which two or more reactants combine to form a single product. These are generally accompanied by the release of heat so they are exothermic reactions.

Example of combination reaction:

${\text{Ba}} + {{\text{F}}_2} \to {\text{Ba}}{{\text{F}}_2}$

2. Decomposition reactions:

The opposite of combination reactions is called a decomposition reaction. Here, a single reactant gets broken into two or more products. Such reactions are usually endothermic because energy is required to break the existing bonds between the reactant molecules.

Example of decomposition reaction:

$2{{\text{H}}_2}{{\text{O}}_2} \to 2{{\text{H}}_2}{\text{O}} + {{\text{O}}_2}$

3. Displacement reactions

Also known as replacement or metathesis reactions. Here, one of the reactants gets replaced by the other one. Generally, the more reactive element displaces the less reactive element. Both metals and non-metals can take part in displacement reactions.

Example of displacement reaction:

${\text{Cu}} + {\text{AgN}}{{\text{O}}_3} \to {\text{Ag}} + {\text{Cu}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}$

4. Double displacement reactions

Double displacement reaction is defined as the reaction in which ions of two compounds interchange with each other to form the product. A general double displacement reaction between two compounds AX and BY can be written as follows:

${\text{AX}} + {\text{BY}} \to {\text{AY}} + {\text{BX}}$

Example of double displacement reaction:

${\text{N}}{{\text{a}}_2}{\text{S}} + {\text{HCl}} \to {\text{NaCl}} + {{\text{H}}_2}{\text{S}}$

5. Combustion reactions:

These are the reactions that take place when hydrocarbons are burnt in the presence of oxygen to form carbon dioxide and water. These are also referred to as burning.

Example of combustion reaction:

${\text{C}}{{\text{H}}_4} + {{\text{O}}_2} \to {\text{C}}{{\text{O}}_2} + {{\text{H}}_2}{\text{O}}$

NaCl reacts with ${\text{H}}{{\text{g}}_{\text{2}}}{\left( {{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_{\text{2}}}} \right)_2}$ to form ${\text{H}}{{\text{g}}_{\text{2}}}{\text{C}}{{\text{l}}_2}$ and ${\text{Na}}{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_2}$ . This is a double displacement reaction that occurs between NaCl and ${\text{H}}{{\text{g}}_{\text{2}}}{\left( {{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_{\text{2}}}} \right)_2}$ . In this reaction, ${\text{C}}{{\text{l}}^-}$ is replaced by ${\left( {{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_{\text{2}}}} \right)^-}$ and products are formed. ${\text{H}}{{\text{g}}_{\text{2}}}{\text{C}}{{\text{l}}_2}$ exists in the solid phase whereas ${\text{Na}}{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{3}}}{{\text{O}}_2}$ is present in aqueous phase.

Learn more:

1. Balanced chemical equation: link

2. Identify the precipitate in the reaction: link

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: Double displacement reaction, combustion reaction, NaCl, Hg2Cl2, Hg2(C2H3O2)2, NaC2H3O2, displacement reaction, combination reaction, decomposition reaction, chemical reactions.

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