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Questions and Answers
Define what an electrochemical cell is?
Define what an electrochemical cell is?
A device that converts chemical energy into electrical energy and vice versa. It consists of two electrodes immersed in one or more suitable electrolytes.
What is the function of the anode in an electrochemical cell?
What is the function of the anode in an electrochemical cell?
What is the role of electrolytes in an electrochemical cell?
What is the role of electrolytes in an electrochemical cell?
Electrolytes are the medium that facilitates the flow of ions between electrodes.
Oxidation and reduction reactions in electrochemical cells occur in separate containers.
Oxidation and reduction reactions in electrochemical cells occur in separate containers.
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Which type of electrochemical cell produces electricity as a result of chemical reactions?
Which type of electrochemical cell produces electricity as a result of chemical reactions?
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Which type of electrochemical cell uses electrical energy to drive chemical reactions?
Which type of electrochemical cell uses electrical energy to drive chemical reactions?
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Which of the following is NOT a function of a salt bridge in an electrochemical cell?
Which of the following is NOT a function of a salt bridge in an electrochemical cell?
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What is the standard notation for representing an Electrochemical Cell?
What is the standard notation for representing an Electrochemical Cell?
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The electrode potential of a cell ONLY depends upon the nature of metal and its ions.
The electrode potential of a cell ONLY depends upon the nature of metal and its ions.
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What is the formula for EMF or cell potential of a cell?
What is the formula for EMF or cell potential of a cell?
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Electrochemical Series arranges elements in increasing order of oxidation potential values.
Electrochemical Series arranges elements in increasing order of oxidation potential values.
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Which of the following is NOT an application of the Electrochemical Series?
Which of the following is NOT an application of the Electrochemical Series?
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What is the Nernst Equation and what does it represent?
What is the Nernst Equation and what does it represent?
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What is the formula for the Nernst Equation?
What is the formula for the Nernst Equation?
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Which of the following is NOT a factor considered in determining the standard electrode potential?
Which of the following is NOT a factor considered in determining the standard electrode potential?
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What is the Nernst Equation used for in the context of electrochemical cells?
What is the Nernst Equation used for in the context of electrochemical cells?
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Study Notes
Electrochemical Cells
- Electrochemical cells convert chemical energy into electrical energy, and vice versa.
- A cell consists of two electrodes immersed in one or more electrolytes.
Electrodes and Electrolytes
- Anode: The electrode where oxidation occurs.
- Cathode: The electrode where reduction occurs.
- Electrolytes: A medium that facilitates the flow of ions between electrodes.
Oxidation and Reduction Reactions
- Oxidation and reduction reactions happen in separate containers not in direct contact.
Galvanic vs. Electrolytic Cells
- Galvanic Cell: Produces electricity from spontaneous chemical reactions inside the cell.
- Electrolytic Cell: Electrical energy drives a chemical reaction (non-spontaneous)
A Simple Galvanic Cell (Daniel Cell)
- Contains a 1.0 M zinc sulfate solution and a 1.0 M copper sulfate solution.
- A zinc rod is dipped in the zinc sulfate solution and a copper rod in the copper sulfate solution.
Reactions at the Anode
- Oxidation occurs at the anode (negative terminal).
- The half-cell where oxidation occurs is known as the oxidation half-cell.
Reactions at the Cathode
- Reduction occurs at the cathode (positive terminal).
- The half-cell where reduction happens is called the reduction half-cell.
Electron Flow in a Galvanic Cell
- Electrons flow from the negative terminal (anode) to the positive terminal (cathode).
- The flow of electrical current is opposite to the flow of electrons.
Functions of Salt Bridge
- Completes the circuit, allowing ions to move between the two half-cells.
- Prevents the mixing of solutions from both half-cells.
- Prevents liquid-junction potential (which is harmful for the cell).
Representation of an Electrochemical Cell
- The anode is written on the left, and the cathode on the right.
- The order is metal/cation//cation/metal (or solid phase then electrolyte).
- A vertical line (/) or semicolon (;) separates the metal from the cation.
- A double line (//) represents the salt bridge.
Electrode Potential and EMF of a Galvanic Cell
- Electrode potential depends on the nature of the metal, the concentration of ions, and temperature.
- EMF (electromotive force) is the difference in electrode potentials between the two electrodes in a cell. It is measured in volts (V). Ecell = Ecathode − Eanode
Electrochemical Series
- An arrangement of elements based on their increasing reduction potential values.
- Also known as the activity series.
- Helpful in predicting spontaneity of a reaction and predicting if a metal will react with acids to produce H₂ gas.
Example Calculations and Predictions
- Examples demonstrate calculating standard EMF of a cell, predicting if reactions are feasible based on electrochemical series, and various applications.
Nernst Equation
- The Nernst equation relates the electrode potential to the concentration of reactants and products and temperature. It accounts for non-standard conditions.
- The equation is: E = E° - (0.0591/n) log[Products]/[Reactants].
Application of Nernst Equation
- Used to calculate cell potentials under non-standard conditions.
Calculation of Cell Potential
- Examples show calculating cell potentials for specific electrochemical cells.
Calculation of Equilibrium Constant
- The equilibrium constant is calculated using the cell potential.
- The equation is K = 10^(nE°/0.0591).
Concentration Determination
- The concentration of one ionic species can be determined if the concentration of the other is known using the Nernst equation.
pH Determination
- The Nernst equation can be used to calculate pH of a solution given the relevant electrochemical cell measurements.
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Description
Test your knowledge on electrochemical cells, including the functions of electrodes, oxidation and reduction reactions, and the differences between galvanic and electrolytic cells. This quiz covers key concepts like the Daniel cell and the reactions occurring at the anode and cathode.
