Electrochemistry - Resistance
Definition of resistance in the context of electrochemistry
Mathematical representation of resistance: R = V/I
Units of resistance: Ohms (Ω)
Factors affecting resistance:
Length and cross-sectional area of the conductor
Temperature of the conductor
Nature and composition of the conductor material
Examples of conductors with high and low resistance
Electrochemistry - Conductance
Definition of conductance in the context of electrochemistry
Mathematical representation of conductance: G = 1/R
Units of conductance: Siemens (S)
Relation between resistance and conductance: G = 1/R
Factors affecting conductance:
Presence of impurities or foreign substances
Temperature of the conductor
Nature and composition of the conductor material
Examples of conductors with high and low conductance
Electrochemistry - Equivalent Conductance
Definition of equivalent conductance in the context of electrochemistry
Mathematical representation of equivalent conductance: Λ = G x V
Units of equivalent conductance: Siemens meter square per mole (S m^2 mol^-1)
Relation between equivalent conductance and conductance: Λ = G x V
Factors affecting equivalent conductance:
Presence of ions in the solution
Temperature of the solution
Nature and concentration of the electrolyte
Examples of electrolytes with high and low equivalent conductance
Electrochemistry - Kohlrausch’s Law
Introduction to Kohlrausch’s Law
Statement of Kohlrausch’s Law
Mathematical representation of Kohlrausch’s Law: ΛΛ = Σ(ν_i * λ_i)
Explanation of terms in the equation
ΛΛ: Equivalent conductance of the electrolyte
ν_i: Stoichiometric coefficient of the ion in the balanced chemical equation
λ_i: Limiting molar conductivity of the ion
Applications of Kohlrausch’s Law in determining the molar conductivity of electrolytes
Electrochemistry - Variation of Conductivity with Concentration
Variation of conductivity with concentration in strong electrolytes
Influence of concentration on dissociation and ionization of strong electrolytes
Influence of concentration on interionic attractions in strong electrolytes
Relation between equivalent conductance and concentration of strong electrolytes
Ionic product of water (K_w) and its significance in conductivity measurements
Electrochemistry - Electrolytic Cells
Introduction to electrolytic cells
Definition of electrolysis
Components of an electrolytic cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
External power source
Working principle of electrolytic cells
Examples of practical applications of electrolytic cells
Electrochemistry - Electrochemical Cells
Introduction to electrochemical cells
Definition of electrochemical reactions
Components of an electrochemical cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
Salt bridge or porous partition
External circuit
Working principle of electrochemical cells
Examples of practical applications of electrochemical cells
Electrochemistry - Galvanic Cells
Introduction to galvanic cells
Definition of galvanic (voltaic) reactions
Principle of operation of galvanic cells: spontaneous redox reactions
Components of a galvanic cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
Salt bridge or porous partition
External circuit
Examples of practical applications of galvanic cells
Electrochemistry - Standard Electrode Potential
Definition of standard electrode potential
Representation of standard electrode potential: E°
Measurement of standard electrode potential using standard hydrogen electrode (SHE)
Comparison of electrode potentials to determine the standard electrode potential of a half-cell
Significance of standard electrode potential in predicting spontaneity of redox reactions
Electrochemistry - Resistance
Definition of resistance in the context of electrochemistry
Mathematical representation of resistance: R = V/I
Units of resistance: Ohms (Ω)
Factors affecting resistance:
Length and cross-sectional area of the conductor
Temperature of the conductor
Nature and composition of the conductor material
Examples of conductors with high and low resistance
Electrochemistry - Conductance
Definition of conductance in the context of electrochemistry
Mathematical representation of conductance: G = 1/R
Units of conductance: Siemens (S)
Relation between resistance and conductance: G = 1/R
Factors affecting conductance:
Presence of impurities or foreign substances
Temperature of the conductor
Nature and composition of the conductor material
Examples of conductors with high and low conductance
Electrochemistry - Equivalent Conductance
Definition of equivalent conductance in the context of electrochemistry
Mathematical representation of equivalent conductance: Λ = G x V
Units of equivalent conductance: Siemens meter square per mole (S m^2 mol^-1)
Relation between equivalent conductance and conductance: Λ = G x V
Factors affecting equivalent conductance:
Presence of ions in the solution
Temperature of the solution
Nature and concentration of the electrolyte
Examples of electrolytes with high and low equivalent conductance
Electrochemistry - Kohlrausch’s Law
Introduction to Kohlrausch’s Law
Statement of Kohlrausch’s Law
Mathematical representation of Kohlrausch’s Law: ΛΛ = Σ(ν_i * λ_i)
Explanation of terms in the equation:
ΛΛ: Equivalent conductance of the electrolyte
ν_i: Stoichiometric coefficient of the ion in the balanced chemical equation
λ_i: Limiting molar conductivity of the ion
Applications of Kohlrausch’s Law in determining the molar conductivity of electrolytes
Electrochemistry - Variation of Conductivity with Concentration
Variation of conductivity with concentration: strong electrolytes
Influence of concentration on dissociation and ionization of strong electrolytes
Influence of concentration on interionic attractions in strong electrolytes
Relation between equivalent conductance and concentration of strong electrolytes
Ionic product of water (K_w) and its significance in conductivity measurements
Electrochemistry - Electrolytic Cells
Introduction to electrolytic cells
Definition of electrolysis
Components of an electrolytic cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
External power source
Working principle of electrolytic cells
Examples of practical applications of electrolytic cells
Electrochemistry - Electrochemical Cells
Introduction to electrochemical cells
Definition of electrochemical reactions
Components of an electrochemical cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
Salt bridge or porous partition
External circuit
Working principle of electrochemical cells
Examples of practical applications of electrochemical cells
Electrochemistry - Galvanic Cells
Introduction to galvanic cells
Definition of galvanic (voltaic) reactions
Principle of operation of galvanic cells: spontaneous redox reactions
Components of a galvanic cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
Salt bridge or porous partition
External circuit
Examples of practical applications of galvanic cells
Electrochemistry - Standard Electrode Potential
Definition of standard electrode potential
Representation of standard electrode potential: E°
Measurement of standard electrode potential using standard hydrogen electrode (SHE)
Comparison of electrode potentials to determine the standard electrode potential of a half-cell
Significance of standard electrode potential in predicting spontaneity of redox reactions
Electrochemistry - Resistance
Definition of resistance in the context of electrochemistry
Mathematical representation of resistance: R = V/I
Units of resistance: Ohms (Ω)
Factors affecting resistance:
Length and cross-sectional area of the conductor
Temperature of the conductor
Nature and composition of the conductor material
Examples of conductors with high and low resistance
Electrochemistry - Conductance
Definition of conductance in the context of electrochemistry
Mathematical representation of conductance: G = 1/R
Units of conductance: Siemens (S)
Relation between resistance and conductance: G = 1/R
Factors affecting conductance:
Presence of impurities or foreign substances
Temperature of the conductor
Nature and composition of the conductor material
Examples of conductors with high and low conductance
Electrochemistry - Equivalent Conductance
Definition of equivalent conductance in the context of electrochemistry
Mathematical representation of equivalent conductance: Λ = G x V
Units of equivalent conductance: Siemens meter square per mole (S m^2 mol^-1)
Relation between equivalent conductance and conductance: Λ = G x V
Factors affecting equivalent conductance:
Presence of ions in the solution
Temperature of the solution
Nature and concentration of the electrolyte
Examples of electrolytes with high and low equivalent conductance
Electrochemistry - Kohlrausch’s Law
Introduction to Kohlrausch’s Law
Statement of Kohlrausch’s Law
Mathematical representation of Kohlrausch’s Law: ΛΛ = Σ(ν_i * λ_i)
Explanation of terms in the equation
ΛΛ: Equivalent conductance of the electrolyte
ν_i: Stoichiometric coefficient of the ion in the balanced chemical equation
λ_i: Limiting molar conductivity of the ion
Applications of Kohlrausch’s Law in determining the molar conductivity of electrolytes
Electrochemistry - Variation of Conductivity with Concentration
Variation of conductivity with concentration in strong electrolytes
Influence of concentration on dissociation and ionization of strong electrolytes
Influence of concentration on interionic attractions in strong electrolytes
Relation between equivalent conductance and concentration of strong electrolytes
Ionic product of water (K_w) and its significance in conductivity measurements
Electrochemistry - Electrolytic Cells
Introduction to electrolytic cells
Definition of electrolysis
Components of an electrolytic cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
External power source
Working principle of electrolytic cells
Examples of practical applications of electrolytic cells
Electrochemistry - Electrochemical Cells
Introduction to electrochemical cells
Definition of electrochemical reactions
Components of an electrochemical cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
Salt bridge or porous partition
External circuit
Working principle of electrochemical cells
Examples of practical applications of electrochemical cells
Electrochemistry - Galvanic Cells
Introduction to galvanic cells
Definition of galvanic (voltaic) reactions
Principle of operation of galvanic cells: spontaneous redox reactions
Components of a galvanic cell:
Electrolyte solution or molten electrolyte
Cathode
Anode
Salt bridge or porous partition
External circuit
Examples of practical applications of galvanic cells
Electrochemistry - Standard Electrode Potential
Definition of standard electrode potential
Representation of standard electrode potential: E°
Measurement of standard electrode potential using standard hydrogen electrode (SHE)
Comparison of electrode potentials to determine the standard electrode potential of a half-cell
Significance of standard electrode potential in predicting spontaneity of redox reactions