Respuesta :
The complete ionic equation for the reaction is as follows:
[tex]\boxed{{{\mathbf{H}}^ + }\left( q \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right) + {\mathbf{O}}{{\mathbf{H}}^ - }\left( {aq} \right) \to {{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left( l \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right)}[/tex]
Further Explanation:
Double displacement reaction is defined as the reaction in which ions of two compound interchange with each other to form the product. For example, the general double displacement reaction between two compounds AX and BY is as follows:
[tex]{\text{AX}} + {\text{BY}} \to {\text{AY}} + {\text{BX}}[/tex]
The three types of equations that are used to represent the chemical reaction are as follows:
1. Molecular equation
2. Complete ionic equation
3. Net ionic equation
The reactants and products remain in undissociated form in molecular equation. In the case of complete ionic equation, all the ions that are dissociated and present in the reaction mixture are represented while in the case of net ionic equation only the useful ions that participate in the reaction are represented.
The steps to write the complete ionic reaction are as follows:
Step 1: Write the molecular equation for the reaction with the phases in the bracket.
In the reaction, HI reacts with RbOH to form RbI and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex]. The balanced molecular equation of the reaction is as follows:
[tex]{\text{HI}}\left( {aq} \right) + {\text{RbOH}}\left( {aq} \right) \to {\text{RbI}}\left( {aq} \right){\text{ + }}{{\text{H}}_{\text{2}}}{\text{O}}\left( l \right)[/tex]
Step 2: Dissociate all the compounds with the aqueous phase to write the complete ionic equation. The compounds with solid and liquid phase remain same. The complete ionic equation is as follows:
[tex]{{\mathbf{H}}^ + }\left( q \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right) + {\mathbf{O}}{{\mathbf{H}}^ - }\left( {aq} \right) \to {{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left( l \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right)[/tex]
Learn more:
1. Balanced chemical equation https://brainly.com/question/1405182
2. Oxidation and reduction reaction https://brainly.com/question/2973661
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Chemical reaction and equation
Keywords: Double displacement reaction, types of equation, molecular equation, complete ionic equation, net ionic equation, RbI, RbOH, H2O, HI, chemical reaction.
The complete ionic equation for the reaction is; H^+(aq) + I^-(aq) + Rb^+(aq) + OH^-(aq) ------> Rb^+(aq) + I^-(aq) + H2O(l)
First, we must write the molecular reaction equation as follows;
HI(aq) + RbOH(aq) -----> RbI(aq) + H2O(l)
Then we write the complete ionic equation as follows;
H^+(aq) + I^-(aq) + Rb^+(aq) + OH^-(aq) ------> Rb^+(aq) + I^-(aq) + H2O(l)
The net ionic equation is now written as;
H^+(aq) + H^-(aq) ------> H2O(l)
The spectator ions occur on both sides of the reaction equation and do not occur in the net ionic equation.
Learn more: https://brainly.com/question/11969651
