Podcast
Questions and Answers
What does the cell reaction in an electrochemical cell represent?
What does the cell reaction in an electrochemical cell represent?
- The reaction occurring exclusively at the anode
- The sum of oxidation and reduction reactions (correct)
- The decomposition of electrolyte solutions
- The total number of electrons lost during oxidation
In the representation of a Galvanic cell, which part indicates the anode half-cell?
In the representation of a Galvanic cell, which part indicates the anode half-cell?
- The entire cell reaction part
- The region between the salt bridge
- The part on the right side of the cell diagram
- The part on the left side of the cell diagram (correct)
What is the significance of the double vertical lines (//) in a cell representation?
What is the significance of the double vertical lines (//) in a cell representation?
- They indicate a potential difference between electrodes
- They indicate the salt bridge between half-cells (correct)
- They separate different phases of the same electrode
- They represent a complete electrochemical cell
Which statement correctly describes the concept of electromotive force (EMF) in an electrochemical cell?
Which statement correctly describes the concept of electromotive force (EMF) in an electrochemical cell?
According to the Nernst equation, what does it relate?
According to the Nernst equation, what does it relate?
What does the zinc half-cell reaction represent in a Galvanic cell?
What does the zinc half-cell reaction represent in a Galvanic cell?
How is the EMF value of a cell typically represented?
How is the EMF value of a cell typically represented?
What formula represents a general cell reaction for the Nernst equation?
What formula represents a general cell reaction for the Nernst equation?
What is the primary function of the salt bridge in an electrochemical cell?
What is the primary function of the salt bridge in an electrochemical cell?
Which type of electrode is typically used to measure the potential of another electrode?
Which type of electrode is typically used to measure the potential of another electrode?
Which electrode is considered to have an electrode potential of 'zero' at all temperatures?
Which electrode is considered to have an electrode potential of 'zero' at all temperatures?
In a galvanic cell, what is the source of electrical energy?
In a galvanic cell, what is the source of electrical energy?
Which of the following represents the reaction at the cathode in the given electrochemical cell?
Which of the following represents the reaction at the cathode in the given electrochemical cell?
Which of the following is NOT a type of electrode mentioned?
Which of the following is NOT a type of electrode mentioned?
Which equation is used to calculate the cell potential (EMF) of an electrochemical cell?
Which equation is used to calculate the cell potential (EMF) of an electrochemical cell?
What does 'n' in the Nernst equation represent?
What does 'n' in the Nernst equation represent?
What type of energy conversion takes place in a galvanic cell?
What type of energy conversion takes place in a galvanic cell?
In a galvanic cell, what is the charge of the anode?
In a galvanic cell, what is the charge of the anode?
Which of the following components is NOT part of a battery?
Which of the following components is NOT part of a battery?
What distinguishes a galvanic cell from an electrolytic cell?
What distinguishes a galvanic cell from an electrolytic cell?
What is a characteristic of galvanic cells?
What is a characteristic of galvanic cells?
What happens to the reactants in a primary battery after it is used?
What happens to the reactants in a primary battery after it is used?
A lithium cell with a solid cathode is known as which type?
A lithium cell with a solid cathode is known as which type?
Which of the following is true about the voltage of a battery during discharge?
Which of the following is true about the voltage of a battery during discharge?
Study Notes
Electrochemical Cells
- An electrochemical cell is a device that converts chemical energy into electrical energy or vice versa.
- Consists of two half-cells: anode (oxidation) and cathode (reduction).
- Cell reaction: Anode half-cell reaction + Cathode half-cell reaction.
- Electrolyte: A solution that conducts electricity due to the movement of ions.
- Salt bridge: A U-shaped tube filled with an electrolyte that connects the two half-cells, maintaining electrical neutrality.
Electromotive Force (EMF)
- EMF or cell potential, is the potential difference required for electron flow from anode to cathode.
- Determined by the difference in potential between the two half-cells and the nature of the electrolyte.
Cell Representation
- Symbolic representation of a cell uses vertical lines (/) and double vertical lines (//) for phase boundaries and the salt bridge, respectively.
- Left side: Anode half-cell.
- Right side: Cathode half-cell.
- Example: Zn/ZnSO4//CuSO4/Cu.
Nernst Equation
- Relates electrode potential to concentration of reactants and products, and temperature.
- Formula: Ecell = Eocell - (0.0591/n) * log (A^a B^b / C^c D^d)
- Where:
Ecellis cell potential.Eocellis standard cell potential.nis the number of electrons transferred.Ris the gas constant.Tis temperature.Fis Faraday's constant.A,B,C, andDare the concentrations of the reactants and products.
Types of Electrochemical Cells
- Galvanic cell (Voltaic cell): Converts chemical energy into electrical energy through spontaneous redox reactions.
- Electrolytic cell: Converts electrical energy into chemical energy.
Reference Electrodes
- Used to determine the electrode potential of another electrode.
- Standard Hydrogen Electrode (SHE): Considered the primary reference electrode and has a potential of 0 Volts at all temperatures.
- Standard Calomel Electrode (SCE): Another commonly used reference electrode.
Batteries
- Collections of cells that store chemical energy and release it as electrical energy.
- Main components: Anode, Cathode, and Electrolyte.
- Characteristics:
- High capacity
- High energy efficiency
- Long shelf life
- Tolerance to different service conditions
- Affordable cost
Types of Batteries
- Primary battery: Non-rechargeable, used only once.
- Examples: Lithium cells, Dry cells.
- Secondary battery: Rechargeable, can be used for multiple cycles.
- Examples: Lead acid storage cells, Lithium-ion cells.
Lithium Cells
- Primary cell: Uses Lithium (Li) as the anode.
- Two types:
- Lithium Cell with Solid Cathode (LSC): Ex: Li-MnO2
- Lithium cell with Liquid Cathode (LLC): Ex: Li-SO2 and Li-SOCl2
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
Test your understanding of electrochemical cells and their components, including the concepts of EMF and cell representation. This quiz covers the basic principles surrounding the conversion of chemical energy into electrical energy, the role of the electrolyte, and the significance of the salt bridge in maintaining cell functionality.
