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Questions and Answers
Which of the following correctly represents the anode notation in a galvanic cell?
Which of the following correctly represents the anode notation in a galvanic cell?
- Metal/Electrolyte (correct)
- Metal/Cation
- Electrolyte/Metal
- Cation/Metal
What does EMF stand for in the context of electrochemical cells?
What does EMF stand for in the context of electrochemical cells?
- Electronic Mass Function
- Electrode Mobility Factor
- Electromotive Force (correct)
- Electrolytic Measurement Frequency
Which of the following factors does NOT affect the electrode potential?
Which of the following factors does NOT affect the electrode potential?
- Nature of metal
- Temperature
- Concentration of ions
- Presence of light (correct)
What is the primary purpose of the electrochemical series?
What is the primary purpose of the electrochemical series?
Which of the following applications of the electrochemical series deals with predicting if a metal can displace another in an acid?
Which of the following applications of the electrochemical series deals with predicting if a metal can displace another in an acid?
How is the standard EMF of a cell calculated?
How is the standard EMF of a cell calculated?
In the equation 2Ag(s) + Zn2+(aq) ⇌ 2Ag+(aq) + Zn(s), which metal is reduced?
In the equation 2Ag(s) + Zn2+(aq) ⇌ 2Ag+(aq) + Zn(s), which metal is reduced?
If an iron wire is placed in a solution of ZnSO4 and NiSO4, which reaction is most likely to occur?
If an iron wire is placed in a solution of ZnSO4 and NiSO4, which reaction is most likely to occur?
What is the standard condition for the concentration of electrolytes in the electrode potential?
What is the standard condition for the concentration of electrolytes in the electrode potential?
In the Nernst equation, what does the term 'n' represent?
In the Nernst equation, what does the term 'n' represent?
What happens to the cell at equilibrium according to the information provided?
What happens to the cell at equilibrium according to the information provided?
What is the equation for calculating the cell potential (E)?
What is the equation for calculating the cell potential (E)?
What is the main use of the Nernst equation?
What is the main use of the Nernst equation?
What is the value of the standard electrode potential (E°) at 298 K?
What is the value of the standard electrode potential (E°) at 298 K?
When calculating the equilibrium constant (K), what must the electrode potential (E) equal at equilibrium?
When calculating the equilibrium constant (K), what must the electrode potential (E) equal at equilibrium?
Which statement correctly defines an electrochemical cell?
Which statement correctly defines an electrochemical cell?
What occurs at the anode of an electrochemical cell?
What occurs at the anode of an electrochemical cell?
In a galvanic cell, what is the primary function of the cathode?
In a galvanic cell, what is the primary function of the cathode?
What is the function of the salt bridge in an electrochemical cell?
What is the function of the salt bridge in an electrochemical cell?
Which type of electrochemical cell converts chemical energy into electrical energy?
Which type of electrochemical cell converts chemical energy into electrical energy?
In a galvanic cell, what is the flow direction of electrons?
In a galvanic cell, what is the flow direction of electrons?
What distinguishes an electrolytic cell from a galvanic cell?
What distinguishes an electrolytic cell from a galvanic cell?
What is the standard notation for an electrochemical cell?
What is the standard notation for an electrochemical cell?
Flashcards
Electrochemical Cell
Electrochemical Cell
A device that converts chemical energy into electrical energy and vice versa. It consists of two electrodes (anode and cathode) immersed in an electrolyte.
Anode
Anode
The electrode at which oxidation occurs. It loses electrons.
Cathode
Cathode
The electrode at which reduction occurs. It gains electrons.
Electrolyte
Electrolyte
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Galvanic Cell
Galvanic Cell
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Electrolytic Cell
Electrolytic Cell
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Daniel Cell
Daniel Cell
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Salt Bridge
Salt Bridge
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Electrode Potential and Concentration
Electrode Potential and Concentration
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Standard Electrode Potential
Standard Electrode Potential
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Nernst Equation
Nernst Equation
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Calculating Cell Potential
Calculating Cell Potential
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Calculating Equilibrium Constant
Calculating Equilibrium Constant
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Applications of the Nernst Equation
Applications of the Nernst Equation
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Electrochemical Series
Electrochemical Series
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EMF (Cell Potential)
EMF (Cell Potential)
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Electrode Potential
Electrode Potential
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Cell Notation
Cell Notation
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Study Notes
Electrochemical Cells
- Electrochemical cells convert chemical energy into electrical energy, or vice versa
- They consist of two electrodes immersed in one or more electrolytes
Electrodes and Electrolytes
- Anode - site of oxidation
- Cathode - site of reduction
- Electrolytes - facilitate ion flow between electrodes
Oxidation-Reduction Reactions
- Oxidation and reduction reactions occur in separate containers, not directly touching
Galvanic vs. Electrolytic Cells
- Galvanic cells produce electricity from spontaneous chemical reactions
- Electrolytic cells use electrical energy to drive non-spontaneous reactions
Simple Galvanic Cell (Daniel Cell)
- Contains 1.0 M ZnSO₄ and 1.0 M CuSO₄ solutions
- A zinc rod dipped in ZnSO₄ solution
- A copper rod dipped in CuSO₄ solution
Reactions at the Anode
- Oxidation occurs at the anode (negative terminal)
- Example: Zn(s) → Zn²⁺(aq) + 2e⁻ (oxidation)
Reactions at the Cathode
- Reduction occurs at the cathode (positive terminal)
- Example: Cu²⁺(aq) + 2e⁻ → Cu(s) (reduction)
Electron Flow in a Galvanic Cell
- Electrons flow from the negative terminal (anode) to the positive terminal (cathode)
- Electric current flows opposite to electron flow
Functions of a Salt Bridge
- Completes the circuit and allows ion flow between half-cells
- Prevents the mixing of solutions
- Prevents liquid-junction potential
Representation of an Electrochemical Cell
- Anode written on left, cathode on right
- Metal/solid phase then electrolyte (cation)
- Separated by a vertical line (/) or semicolon (;)
- Salt bridge represented by double lines (//)
Electrode Potential and EMF of a Galvanic Cell
- Electrode potential depends on the nature of the metal, concentration of ions, and temperature
- EMF is the difference in electrode potential between two electrodes, expressed in volts (V)
- Ecell = Ecathode - Eanode
Electrochemical Series
- Arrangement of elements based on increasing reduction potentials (activity series)
- Used to predict oxidizing/reducing agent strength, spontaneity of reactions, metal reactivity with acids, and replacement tendencies
Nernst Equation
- Relates electrode potential (E) to standard electrode potential (E°), concentrations of species, and temperature
- E = E° - (0.0591/n) log ([products]/[reactants])
Calculation of Cell Potential
- Calculate potential for each half-cell and total EMF (use Nernst equation)
Calculation of Equilibrium Constant
- At equilibrium, ΔG = 0
- Ecell = 0, use the Nernst equation to calculate equilibrium constant (K)
Concentration Determination
- Calculate the concentration of one ionic species if concentration of other species is known, using the Nernst equation
pH Determination
- Calculate pH of a solution by using the Nernst equation and the known values of electrodes
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Description
Explore the fundamentals of electrochemical cells, including the functions of electrodes and electrolytes. This quiz covers oxidation-reduction reactions, the distinctions between galvanic and electrolytic cells, and the specifics of a simple galvanic cell like the Daniel Cell.
