Respuesta :
STANDARD CELL NOTATION:
1. The anode is always written in the left side of the ||
2. States are separated by a |; species of a common state are separated by a comma
3. The salt bridge is represented by ||
I think the correct notation would be:
Pb(s) | PbCl2(s) | Cl-(aq) || Cl-(aq) | AgCl2(s) | Ag(s)
1. The anode is always written in the left side of the ||
2. States are separated by a |; species of a common state are separated by a comma
3. The salt bridge is represented by ||
I think the correct notation would be:
Pb(s) | PbCl2(s) | Cl-(aq) || Cl-(aq) | AgCl2(s) | Ag(s)
The cell notation is [tex]\boxed{{\text{Pb}}\left( {\text{s}} \right){\text{,PbC}}{{\text{l}}_2}\left( {\text{s}} \right)|{\text{C}}{{\text{l}}^ - }\left( {{\text{aq}}} \right)||{\text{C}}{{\text{l}}^-}\left({{\text{aq}}}\right)|{\text{AgCl}}\left({\text{s}}\right),{\text{Ag}}\left({\text{s}}\right)}[/tex].
Further explanation
Redox reaction:
Redox is a term that is used collectively for the reduction-oxidation reaction. It is a type of chemical reaction in which the oxidation states of atoms are changed. In this reaction, both reduction and oxidation are carried out simultaneously. Redox reactions are generally characterized by the transfer of electrons between the species involved in the reaction.
The process of gain of electrons or the decrease in the oxidation state of the atom is called reduction while that of loss of electrons or the increase in the oxidation number is known as oxidation. In redox reactions, one species lose electrons, and the other species gain electrons. The species that lose electrons and itself gets oxidized is called as a reductant or reducing agent. The species that gains electrons and gets reduced is known as oxidant or oxidizing agent. The presence of a redox pair or redox couple is a must for the redox reaction.
The general representation of a redox reaction is,
[tex]{\text{X}}+{\text{Y}}\to{{\text{X}}^+}+{{\text{Y}}^-}[/tex]
The oxidation half-reaction can be written as,
[tex]{\text{X}}\to{{\text{X}}^+}+{e^-}[/tex]
The reduction half-reaction can be written as,
[tex]{\text{Y}}+{e^-}\to{{\text{Y}}^-}[/tex]
The oxidation occurs at anode, and the reduction takes place at cathode.
Electrochemical cell is a device which either generates electricity from chemical reaction or causes an unfavorable chemical reaction to occur from electricity. The cell in which electric current is generated from chemical reaction is known as Daniel cell and galvanic cell.
In galvanic cell, the movement of electrons is from anode to cathode. Anode is negatively charged electrode and cathode is positively charged electrode in galvanic cell.
Cell notation is a shorthand hand notation to write redox reaction of a cell. Anode and cathode electrode in electrochemical cell is called as half cells.
Steps to write cell notation are as follows:
Step1: The two half cells are separated by double vertical lines (||). The double vertical lines represent the salt bridge.
Step2: The cell at which oxidation occurs is written on the left side and the cell at which reduction occurs is written on the right side.
Step3: On the same side, two different states of matter in an electrode is separated by single vertical line(|) and different compound having same physical state is separated by comma (,).
Given AgCl is the cathode and[tex]{\text{PbC}}{{\text{l}}_2}[/tex]is anode.
The reduction reaction for AgCl is as follows:
[tex]{\text{AgCl}}\left({\text{s}}\right)+{{\text{e}}^-}\to{\text{Ag}}\left({{\text{aq}}}\right)+{\text{C}}{{\text{l}}^-}\left({{\text{aq}}} \right)[/tex] …… (1)
The oxidation reaction for [tex]{\text{PbC}}{{\text{l}}_2}[/tex]is written as:
[tex]{\text{PbC}}{{\text{l}}_2}\left({\text{s}}\right)+{\text{2}}{{\text{e}}^-} \to {\text{Pb}}\left( {\text{s}}\right)+{\text{2C}}{{\text{l}}^-}\left({{\text{aq}}}\right)[/tex] …… (2)
Multiply equation (1) by 2 to balance number of electrons.
[tex]{\text{2AgCl}}\left( {\text{s}} \right) + {\text{2}}{{\text{e}}^ - } \to {\text{2Ag}}\left( {\text{s}}\right)+{\text{2C}}{{\text{l}}^-}\left({{\text{aq}}}\right)[/tex] ……. (3)
The cell notation for the cell can be written as follows:
[tex]{\mathbf{Pb}}\left( {\mathbf{s}} \right){\mathbf{,PbC}}{{\mathbf{l}}_{\mathbf{2}}}\left( {\mathbf{s}} \right){\mathbf{|C}}{{\mathbf{l}}^-}\left( {{\mathbf{aq}}} \right){\mathbf{||C}}{{\mathbf{l}}^-}\left({{\mathbf{aq}}} \right){\mathbf{|AgCl}}\left( {\mathbf{s}} \right){\mathbf{,Ag}}\left({\mathbf{s}}\right)[/tex]
Learn more:
1. Complete and balance the following equation https://brainly.com/question/5526988
2. Write the net ionic equation https://brainly.com/question/5817505
Answer details:
Grade: Senior school
Subject: Chemistry
Chapter: Redox reaction
Keywords: Oxidation, reduction, chemical reaction, gains, electrons, half cells, electrochemical cell, cell notation, transfer of electrons, Pb, PbCl2, Cl, ag and AgCl2.
